The number of moles of the gas sample present at the end is 0.78 moles.
Number of moles of the gas
PV = nRT
V = nRT/P
At a constant volume, V;
n₁RT₁/P₁ = n₂RT₂/P₂
n₁T₁/P₁ = n₂T₂/P₂
n₂ = (n₁T₁P₂)/(P₁T₂)
where;
T₁ is initial temperature = 21.7⁰C = 294.7 KT₂ is final temperature = 28.1⁰C = 301.1 Kn₂ = (3 x 294.7 x 0.998)/(3.75 x 301.1)
n₂ = 0.78 moles
Thus, the number of moles of the gas sample present at the end is 0.78 moles.
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How many grams of Aspirin (acetylsalicylic acid) should we form in this reaction if we started with 2.08g of Salicyclic Acid?
Taking into account the reaction stoichiometry, 2.713 grams of aspirin are formed when 2.08 grams of salicyclic acid reacts.
Reaction stoichiometryIn first place, the balanced reaction is:
C₄H₆O₃ + C₇H₆O₃ (Salicyclic Acid) →C₉H₈O₄ (aspirin) + C₂H₄O₂
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
C₄H₆O₃: 1 moleC₇H₆O₃: 1 moleC₉H₈O₄: 1 moleC₂H₄O₂: 1 moleThe molar mass of the compounds is:
C₄H₆O₃: 102 g/moleC₇H₆O₃: 138 g/moleC₉H₈O₄: 180 g/moleC₂H₄O₂: 60 g/moleThen, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
C₄H₆O₃: 1 mole ×102 g/mole= 102 gramsC₇H₆O₃: 1 mole ×138 g/mole= 138 gramsC₉H₈O₄: 1 mole ×180 g/mole= 180 gramsC₂H₄O₂: 1 mole ×60 g/mole= 60 gramsMass of aspirin formedThe following rule of three can be applied: if by reaction stoichiometry 138 grams of salicyclic acid form 180 grams of aspirin, 2.08 grams of salicyclic acid form how much mass of aspirin?
[tex]mass of aspirin=\frac{2.08 grams of salicyclic acidx 180 grams of aspirin}{138 grams of salicyclic acid}[/tex]
mass of aspirin= 2.713 grams
Then, 2.713 grams of aspirin are formed when 2.08 grams of salicyclic acid reacts.
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Question 22 (Essay Worth 8 points)
(03.07 MC)
Describe the properties of carbon that makes it possible for millions of carbon compounds to occur naturally.
X5
Source ✔ C
G9
C3H8O dissolved in water
If C3H8O is dissolved in water, it would be expected to be a strong electrolyte.
What is a strong electrolyte?
A strong electrolyte is a solute or solution (already an electrolyte) that can completely dissociates in solution.
C3H8O is one of those compounds expected to be a strong electrolyte.
Thus, if C3H8O is dissolved in water, it would be expected to be a strong electrolyte.
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Predict the products of the double replacement reactions given. Check to see that the equations are
balanced.
AgNO3 + NaCl → ?
O AgNa+CINO3
NaNO3 + AgCl (s)
O 2NaNO3 + 3AgCl (s)
O Ag + NaNO3
Answer:
Option (2)
Explanation:
The two compounds formed will be AgCl and NaNO₃.
We can see that this will result in a balanced equation, so the answer is Option (2).
Answer:
B) NaNO3 + AgCl (s)
Explanation:
edge 2023
What is the molality of lithium ions in a 0.302 m solution of Li₃PO₄ assuming the compound dissociates completely?
The molality of the lithium ions is calculated as 0.906 m
What is the molality of lithium ions?Given that the compound is written as Li₃PO₄, the dissociation of the compound is given by the equation;
Li₃PO₄ -----> 3Li^+ + PO₄^3-
Since there are three mole of lithium ions in the compound, it the follows that the molality of the lithium ions is;
3 * 0.302 m = 0.906 m
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Two isotopes of lithium are found in nature Li6 has a mass of 6. 02u and Li7 has a mass of 7.02u . Use the atomic weight of lithium found on the periodic table to determine which isotope is more abundance
The isotope that is more abundant, given the data is isotope Li7
AssumptionLet Li6 be isotope ALet Li7 be isotope BHow to determine whiche isotope is more abundantMolar mass of isotope A (Li6) = 6.02 uMolar mass of isotope B (Li7) = 7.02 uAtomic mass of lithium = 6.94 uAbundance of A = A%Abundance of B = (100 - A)%Atomic mass = [(mass of A × A%) / 100] + [(mass of B × B%) / 100]
6.94 = [(6.02 × A%) / 100] + [(7.02 × (100 - A)) / 100]
6.94 = [6.02A% / 100] + [702 - 7.02A% / 100]
6.94 = [6.02A% + 702 - 7.02A%] / 100
Cross multiply
6.02A% + 702 - 7.02A% = 6.94 × 100
6.02A% + 702 - 7.02A% = 694
Collect like terms
6.02A% - 7.02A% = 694 - 702
-A% = -8
A% = 8%
Thus,
Abundance of B = (100 - A)%
Abundance of B = (100 - 8)%
Abundance of B = 92%
SUMMARY
Abundance of A (Li6) = 8%Abundance of B (Li7) = 92%From the above, isotope Li7 is more abundant.
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What is common to solving all mola mass problems?
All you need to do is to follow these 3 steps.
1. Estimate the number of each kind of atom present in the compound using the chemical formula in order to determine the molar mass of the molecule.
Divide each element's atomic weight (found in the periodic table) by the quantity of that element's atoms in the compound.Add up the total, then follow the number with the units of grams/mole.eg. Water
2 hydrogen atoms and 1 oxygen atom make up the chemical formula H20.H- 1's atomic weightO-16's atomic weightNumber of H atoms overall in formula 2Number of O atoms overall in formula 1The molar mass will thus be as follows: H 2 x 1= 2 O 1 x 16= 16 16+2= 18Water's molar mass is 18 g/mol as a result.Students in a chemistry lab are making the compound cobalt(II) carbonate.
It can be made by reacting sodium carbonate solution with cobalt(II) chloride solution. Calculate the volume of 2.0 mol/L cobalt(II) chloride solution required to completely react with 250 mL of 1.5 mol/L sodium carbonate.
The volume of 2.0 mol/L cobalt(II) chloride solution required for the reaction is 187.5 mL
How to determine the mole of Na₂CO₃ in the solutionVolume of Na₂CO₃ = 250 mL = 250 / 1000 = 0.25 LMolarity of Na₂CO₃ = 1.5 mol/LMole of Na₂CO₃ = ?Mole = molarity × volume
Mole of Na₂CO₃ = 1.5 × 0.25
Mole of Na₂CO₃ = 0.375 mole
How to determine the mole of CoCl₂ neededBalanced equation
CoCl₂ + Na₂CO₃ -> CoCO₃ + 2NaCl
From the balanced equation above,
1 mole of Na₂CO₃ reacted with 1 mole of CoCl₂.
Therefore,
0.375 mole of Na₂CO₃ will also react with 0.375 mole of CoCl₂.
How to determine the volume of CoCl₂Molarity of CoCl₂ = 2 mol/LMole of CoCl₂ = 0.375 moleVolume of CoCl₂ = ?Volume = mole / molarity
Volume of CoCl₂ = 0.375 / 2
Volume of CoCl₂ = 0.1875 L
Multiply by 1000 to express in mL
Volume of CoCl₂ = 0.1875 × 1000
Volume of CoCl₂ = 187.5 mL
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S + 6 HNO3 --> H₂SO4 + 6 NO₂ + 2 H₂O In the above equation how many moles of H₂SO4 can be made when 7 moles of HNO3 are consumed?
Answer:
1.17 moles H₂SO₄
Explanation:
To find the moles H₂SO₄, you need to multiply the given value by the mole-to-mole ratio. This ratio is made up of the coefficients of the relevant molecules from the balanced chemical equation. It is important to arrange the ratio in a way that allows for the cancellation of units.
S + 6 HNO₃ ------> 1 H₂SO₄ + 6 NO₂ + 2 H₂O
^ ^
7 moles HNO₃ 1 mole H₂SO₄
----------------------- x ------------------------ = 1.17 moles H₂SO₄
6 moles HNO₃
What volume would 20.0 moles of sulfur
dioxide occupy at 75.3 °C with a pressure of
3.50 atm? Answer is in L
Answer:
163 L
Explanation:
To find the volume, you need to use the Ideal Gas Law. The equation looks like this:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = constant (0.0821 L*atm/mol*K)
-----> T = temperature (K)
Before you can plug the given values into the equation, you first need to convert Celsius to Kelvin.
P = 3.50 atm R = 0.0821 L*atm/mol*K
V = ? L T = 75.3 °C + 273.15 = 348.45 K
n = 20.0 moles
PV = nRT
(3.50 atm)V = (20.0 moles)(0.0821 L*atm/mol*K)(348.45 K)
(3.50 atm)V = 572.1549
V = 163 L
ALab Data
78°F
Verify your volume measurement
You have not titrated to the endpoint
Did you report your data to the correct number of
significant figures?
Standardized NaOH (M) 0.4171
Initial volume of buret (mL) 0.50
Volume of vinegar (mL) 10.00
Observations
solution increased.
Final volume of buret (mL)
Volume of NaOH (mL)
Molarity of acetic acid (M)
The correct number of significant figures are,
Final volume of burette is 38.86ml
Volume of NaOH is 38.36ml
Given data:Initial volume of burette V(I)= 0.50ml
Molarity of NaOH is M1 = 0.4171M
Volume of Vinegar V2 = 10.00ml
Molarity of acetic acid M2= 1.6M
Final volume of burette V(f)= ?
volume of NaOH V1 = V(f) - V(I) = ?
Determining the moles of acetic acid (CH3COOH)Molarity = moles of solute / volume of solution
Molarity of acetic acid = moles of CH3C00H / Volume of vinegar
1.6 = moles of CH3C00H / 10.00
moles of CH3C00H = 1.6 * 10.00
Moles of CH3COOH is 16.00mols
Determining the moles of Sodium Hydroxide (NaOH)In a volumetric titration the amount of Standard solution (titrant) used in the titration is stoichiometrically equivalent to amount of unknown solution (analyte) used for the titration at the endpoint.
Hence,
Moles of NaOH = Moles of CH3COOH
Moles of NaOH is 16.00mols
Determining the volume of Sodium Hydroxide (NaOH)Molarity of NaOH = moles of NaOH / Volume of NaOH
0.4171 = 16.00 / V(f)-V(I)
0.4171 = 16.00 / V(f)- 0.50
V(f) = ( 16 / 0.4171 ) + 0.50
V(f) = 38.86 ml
Final volume of NaOH V(f) is 38.86ml
Volume of NaOH V1 = 38.86 - 0.50
Volume of NaOH is 38.36ml
DISCLAIMER: Question is incomplete
Initial volume of burette = 0.50ml
Molarity of NaOH = 0.4171M
Volume of Vinegar = 10.00ml
Molarity of acetic acid = 1.6M
Final volume of burette = ?
volume of NaOH = ?
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What color does red cabbage juice make when mixed with a dishwasher soap?
Answer:
Blue or green
Explanation:
A chemical called anthocyanin is in red cabbage juice, which changes color depending on the pH of its environment. Dishwasher soap is usually alkaline, making the juice turn a blue-green color.
27.2 kg of a solution containing 18.7 % KCl by mass
Express your answer in kilograms using three significant figures.
The amount of potassium chloride (KCl) in 27.2 kg of a solution containing 18.7% KCl by mass solution is 5.086 kg.
How to find the mass of solute ?Mass of solute = Mass percent of solute x Mass of the solution
Here,
Mass percent of solute = 18.7 %
Mass of the solution = 27.2 kg
Now put the value in above formula we get
Mass of solute = Mass percent of solute x Mass of the solution
= [tex]\frac{18.7}{100} \times 27.2\ kg[/tex]
= [tex]\frac{508.64}{100}[/tex]
= 5.086
Thus from the above conclusion we can say that The amount of potassium chloride (KCl) in 27.2 kg of a solution containing 18.7% KCl by mass solution is 5.086 kg.
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which gas law is not included in the combined gas law
Answer:
Watson law is not part of the combined gas law
There are 5 basic gas laws of ideal gases:
Boyle's Law: volume (V) is inversely proportional to pressure (P)Charles' Law: V is proportional to temperature (T)Gay-Lussac's Law: P is proportional to TDalton's Law: The total pressure exerted by a mixture of ideal gases is equal to the sum of the pressures of the individual gasesAvogadro's Law: All equal volumes of ideal gases contain the same number of gas particles (at constant T and P); V is proportional to moles (n)The Combined Gas LawThis law features Charles', Boyle's and Gay-Lussac's laws.
Therefore, Dalton's and Avogadro's laws are exluded.
A gaseous compound containing hydrogen and carbon is decomposed and found to contain 90.00% carbon and 10.00% hydrogen by mass. The mass of 371 mL of the gas, measured at 415 mm Hg and 41°C, is found to be 0.315 g. What is the molecular formula of the compound?
The molecular formula of the compound is C₃H₄.
What is the molecular formula of the compound?The molecular formula of the compound is determined from the molecular mass of the compound.
The molecular mass of the compound is derived using the general gas equation as follows:
P₁V₁/T₁ = P₂V₂/T₂
V₂ = P₁V₁T₂/P₂T₁
Volume at STP, V₂ = (415 * 371 * 298(760 * 314)
V₂ = 192.26 mL = 0.192 L
Molar mass of gas = 22.4/0.192 * 0.315 = 36.75 g
Molecular formula is then determined from the mole ratio of the elements;
Carbon = 0.9 * 36.75/12 = 3
Hydrogen = 0.1 * 40/1 = 4
Thus, the molecular formula of the compound is C₃H₄.
In conclusion, the molecular formula of the gas is derived from the molecular mass.
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which best describes the source of radiation heat
A.two molecules colliding with each other
B.Objects having kinetic energy because of their motion
C.Liquid or gas circulating to move the heat
D.The Sun sending out electromagnetic waves
The sun sending out electromagnetic waves is best describes the source of radiation heat.
Radiation heat is the form of electromagnetic waves.
Radiation heat, commonly referred to as thermal radiation, is the electromagnetic radiation that defines how photons exchange heat. The technique of heat transfer known as radiant heat does not require a medium to be propagated in.
Two molecules colliding with each other produce kinetic energy, moving objects have kinetic energy. Radiation heat is thermal energy. Sun directly sends thermal radiation through electromagnetic waves.
Hence , The sun sends out electromagnetic waves directly is best describes the source of radiation heat.
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Identify the potential products NH4Cl+NaClO3
Answer:
NH₄ClO₃ and NaCl
Explanation:
This appears to be a double-displacement reaction. In these reactions, the cation of one compound is swapped with the cation of another.
So, NH₄⁺ from NH₄Cl is swapped with Na⁺ from NaClO₃. It is important that the resulting ionic compound has an overall charge of 0. In this case, the charges perfectly balance, so there only needs to be one atom of each ion in the compounds.
1.) NH₄ClO₃
-----> NH₄⁺ and ClO₃⁻
-----> +1 + (-1) = 0
2.) NaCl
-----> Na⁺ and Cl⁻
-----> +1 + (-1) = 0
The chemical equation:
NH₄Cl + NaClO₃ -----> NH₄ClO₃ + NaCl
Order the following chemicals from lowest to highest melting point.
Tungsten
Copper (II) chloride
• Caffeine
• Lead
• Sodium chloride
• Silver
Caffeine - Lead (Pb) - Copper (II) chloride (CuCl2) - Sodium chloride (NaCl) - Silver (Ag) - Tungsten
A gas company in Massachusetts charges $1.30 for 17.0ft³ of natural gas. Convert this rate to dollars
per liter of gas.
Answer:
See below
Explanation:
Conversion factor : 1 ft^3 = 28 .317 liters
$ 1.30 /( 17 ft^3 * 28.317 liters/ft^3) = $.0027 per liter
Given the reaction below, how many liters of oxygen are formed if 77.37 L of water are produced at STP? (4pts)
2C4H10 (g) + 13O2 (g) → 8CO2 (g) + 10H2O (g)
Round your answer to two decimal places.
1.2 x 10² L of oxygen is formed if 77.37 L of water is produced.
The density of water at STP = 0.99 g/ ml but we will assume 1 g/ml
Determine the mass of water ([tex]H_{2}[/tex]o) = 77.37 L × [tex]\frac{1000 ml}{1l}[/tex] × [tex]\frac{1g}{ml}[/tex]
The mass of water = 77370 g
Convert mass into moles = 77370 [tex]H_{2}[/tex]o × [tex]\frac{1mol}{18.01528} H _{2}O[/tex]
= 4294.6876 mol of [tex]H_{2} O[/tex]
Use stoichiometry to find how many mols of oxygen [tex]o_{2}[/tex] were used:
= 4294.6876 mol of [tex]H_{2} O[/tex] × [tex]\frac{13 mol }{10 mol}[/tex]
= 5583.0939 mol [tex]o_{2}[/tex]
Convert mols to mass = 5583.0939 mol ×[tex]\frac{32 g}{mol }[/tex]
= 178659.0059 g [tex]o_{2}[/tex]
Convert mass into liters
The density of [tex]o_{2}[/tex] at STP = [tex]\frac{1.439}{ml}[/tex]
Density of [tex]o_{2}[/tex] = 1.2 × [tex]10^{2}[/tex]
Hence,1.2 x 10² L of oxygen is formed if 77.37 L of water is produced.
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1.2 x 10² L of oxygen is formed if 77.37 L of water are produced at STP. The term is derived from the Greek word "oxy genes," which means "forms acid." a periodic table column that is vertical.
What is oxygen ?
The chemical element oxygen has an atomic number of 8. At normal temperatures and pressures, oxygen transforms into the chemical compound (O2) of two atoms, which is a colorless gas.
The density of H₂O at STP = 0.99 g ÷ ml, but we will assume 1 g/ml
The mass of H₂O = 77370 g
Use stoichiometry to find moles of oxygen given by
= 4294.6876 mol of X
= 5583.0939 mol
Convert moles into mass = 5583.0939 mol X
= 178659.0059 g
Then convert it into liter. 1.2 x 10² L of oxygen is formed if 77.37 L of water.
Thus, 1.2 x 10² L of oxygen is formed if 77.37 L of water are produced at STP.
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Calculate the amount of heat deposited on the skin of a person burned by 1.00g of steam at 100.0C. Skin temperature is 37C. ΔHvap= 40.7kJ/mol.
The amount of heat deposited on the skin is 2.26 kJ.
What is the amount of heat given off by 1.0 g of steam?The amount of heat given off by steam is determined using the formula below:
Quantity of heat = mass * latent heat of vaporization.
Moles of steam = 1.0/18
Heat = 1.0/18 * 40.7
Heat deposited = 2.26 kJ
In conclusion, the quantity of heat is determined from the latent heat of vaporization and the moles of steam.
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A rock displaces 1.65 L of water. The volume of the rock is:
Answer:
If a rock displaces 1.65L of water, its volume must be 1.65L.
If you want to convert that to cm^3 it's 1000 cm^3 per liter...so 1650 cm^3
Explanation:
Research the ecology of your region and find one species that is endangered. Find an estimate of the population of the species in your region. Describe the threats facing that species, especially threats posed by human activities.
The endangered species in my region with their estimate population are:
Northwestern African Cheetah - 250 West African Lion - 400 What threat faces Northwestern African Cheetah?This cheetah is said to be an endangered species because of their loss of their habitat and also due to fragmentation, trade and little human-activities.
West African Lion is said to be an endangered species because the lion's historic range in West Africa was said to be lowered by a lot of amount or scale as a result of land use changes and human activities such as falling of trees, buildings, etc.
Hence the endangered species in my region with their estimate population are:
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The heat from the bonfire is transferred to the student's hands through the process of
conduction
convection
radiation
reflection
Answer:
Radiation
Explanation:
Allowing water to cascade or bubble in a fountain during the purification process is an example of
a chemical reaction
O a solid dissolving in a liquid
O only a and b
O ion exchange
O a gas dissolving in a liquid
Answer:
ion exchange
Explanation:
because in the time period of chemical reactions it product ion
If a sample of helium gas at 880 torr and 23°C is allowed to expand from 2.4 L to 5.6 L without changing the temperature, what pressure will the helium gas exert?
275 torr
962 torr
2.01 x 103 torr
377 torr
Answer: 962 torr
Explanation:
A drop of water with a mass of 0.48 g is vaporized at 100 ∘C and condenses on the surface of a 55- g block of aluminum that is initially at 25 ∘C . If the heat released during condensation goes only toward heating the metal, what is the final temperature in Celsius of the metal block? (The specific heat capacity of aluminum is 0.903 J/(g⋅∘C ).)
Express the temperature in Celsius to two significant figures.
The final temperature in Celsius of the metal block is 49°C.
How to find the number of moles ?Moles water = [tex]\frac{\text{Given mass}}{\text{Molar Mass}}[/tex]
= [tex]\frac{0.48\ g}{18\ \text{g/mol}}[/tex]
= 0.0266 moles
Heat lost by water = 0.0266 mol x 44.0 kJ/mol
= 1.17 kJ
= 1170 J [1 kJ = 1000 J]
Heat lost = Heat gained
Heat gained by aluminum = 1170 J
1170 = 55 x 0.903 (T - 25) = 49.7 T - 1242
1170 + 1242 = 49.7 T
T = 48.5°C (49°C at two significant figures)
Thus from the above conclusion we can say that The final temperature in Celsius of the metal block is 49°C.
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What is the molar mass of an unknown gas
with a density of 4.95 g/L at 1.00 atm and
25.0 °C?
Answer:
121 g/mol
Explanation:
To find the molar mass, you first need to calculate the number of moles. For this, you need to use the Ideal Gas Law. The equation looks like this:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = constant (0.0821 L*atm/mol*K)
-----> T = temperature (K)
Because density is comparing the mass per 1 liter, I am assuming that the system has a volume of 1 L. Before you can plug the given values into the equation, you first need to convert Celsius to Kelvin.
P = 1.00 atm R = 0.0821 L*atm/mol*K
V = 1.00 L T = 25.0. °C + 273.15 = 298.15 K
n = ? moles
PV = nRT
(1.00 atm)(1.00L) = n(0.0821 L*atm/mol*K)(298.15 K)
1.00 = n(0.0821 L*atm/mol*K)(298.15 K)
1.00 = (24.478115)n
0.0409 = n
Now, we need to find the molar mass using the number of moles per liter (calculated) and the density.
0.0409 moles ? grams 4.95 grams
---------------------- x ------------------ = ------------------
1 L 1 mole 1 L
? g/mol = 121 g/mol
**note: I am not 100% confident on this answer
Using the balanced equation below.
how many grams of cesium fluoride
would be required to make 73.1 g
of
cesium xenon heptafluoride?
CSF + XeF6 - CsXeF7
A
Answer:
28.0 grams CsF
Explanation:
To find the mass of CsF, you need to (1) convert grams CsXeF₇ to moles CsXeF₇ (via molar mass), then (2) convert moles CsXeF₇ to moles CsF (via mole-to-mole ratio from equation coefficients), and then (3) convert moles CsF to grams CsF (via molar mass). It is important to arrange the ratios/conversions in a way that allows for the cancellation of units. The final answer should have 3 sig figs to match the sig figs of the given value.
Molar Mass (CsF): 132.91 g/mol + 18.998 g/mol
Molar Mass (CsF): 151.908 g/mol
Molar Mass (CsXeF₇): 132.91 g/mol + 131.29 g/mol + 7(18.998 g/mol)
Molar Mass (CsXeF₇): 397.186 g/mol
1 CsF + XeF₆ -----> 1 CsXeF₇
73.1 g CsXeF₇ 1 mole 1 mole CsF 151.908 g
---------------------- x -------------------- x ------------------------ x ------------------ =
397.186 g 1 mole CsXeF₇ 1 mole
= 27.958 g CsF
= 28.0 g CsF
Consider the balanced equation:
Mg2Si (s) + 2 H2O (l) ---> 2 Mg(OH)2 (aq) + SiH4 (g)
Calculate the grams of silane gas, SiH4, formed when 8.48 g of Mg2Si react with excess H2O.
2. Consider the balanced equation:
4 NH3 (g) + 7 O2 (g) ---> 4 NO2 (g) + 6 H2O (g)
What is the mass of H2O produced when 109.4 g of NH3 is completely reacted
1. The mass of silane gas, SiH₄ formed from the reaction is 3.57 g
2. The mass of H₂O produced from the reaction is 173.75 g
1. How to determine the mass of SiH₄ formedBalanced equation
Mg₂Si (s) + 4H₂O (l) ---> 2Mg(OH)₂ (aq) + SiH₄ (g)
Molar mass of Mg₂Si = (24×2) + 28 = 76 g/mol
Mass of Mg₂Si from the balanced equation = 1 × 76 = 76 g
Molar mass of SiH₄ = 28 + (4×1) = 32 g/mol
Mass of SiH₄ from the balanced equation = 1 × 32 = 32 g
SUMMARY
From the balanced equation above,
76 g of Mg₂Si reacted to produce 32 g of SiH₄
From the above information, we can obtain the mass of SiH₄ produced by the reaction of 8.48 g of Mg₂Si as illustrated below:
From the balanced equation above,
76 g of Mg₂Si reacted to produce 32 g of SiH₄
Therefore,
8.48 g of Mg₂Si will react to produce = (8.48 × 32) / 76 = 3.57 g of SiH₄
Thus, 3.57 g of SiH₄ were obtained from the reaction.
2. how to determine the mass of H₂O producedBalanced equation
4NH₃ (g) + 7O₂ (g) ---> 4NO₂ (g) + 6H₂O (g)
Molar mass of NH₃ = 14 + (1×3) = 17 g/mol
Mass of NH₄ from the balanced equation = 4 × 17 = 68 g
Molar mass of H₂O = (2×1) + 16 = 18 g/mol
Mass of H₂O from the balanced equation = 6 × 18 = 108 g
SUMMARY
From the balanced equation above,
68 g of NH₃ reacted to produce 108 g of H₂O
From the above information, we can obtain the mass of H₂O produced by the reaction of 109.4 g of NH₃ as illustrated below:
From the balanced equation above,
68 g of NH₃reacted to produce 108 g of H₂O
Therefore,
109.4 g of NH₃ will react to produce = (109.4 × 108) / 68 = 173.75 g of H₂O
Thus, 173.75 g of H₂O were obtained from the reaction.
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