Answer:
Density = 0.67 g/mLExplanation:
The density of a substance can be found by using the formula
[tex]Density = \frac{mass}{volume} [/tex]To calculate the Density in g/mL we must first convert the mass from kg to g and the volume from L to mL
For the mass
That's
1.34 kg
1kg = 1000 g
1.34 kg = 1000 × 1.34 = 1340 g
For the volume
That's
2.0 L
1 L = 1000 mL
2.0 L = 2 × 1000 = 2000 mL
So we have
mass = 1340 g
volume = 2000 mL
Substitute the values into the above formula and solve for the Density
That's
[tex]Density = \frac{1340}{2000} \\ = \frac{67}{100} [/tex]We have the final answer as
Density = 0.67 g/mLHope this helps you
How does soil structure affect the characteristics of soil? a. It determines the acidity of soil. b. It determines the available nutrients of soil. c. It determines the pore space within soil horizons. d. It determines the amount of minerals present in soil. Please select the best answer from the choices provided A B C D
Answer:
B
Explanation:
Soil structure affects water and air movement in a soil, nutrient availability for plants, root growth, and microorganism activity. ... This allows for greater air and water movement and better root growth.
Answer:
b
Explanation:
Look up the molecular weight of Lithium diisoproylamine and determine the amount of g of base needed for this experiment. Round to the hundredths place
Answer:
0.72 g
Explanation:
Note that, the mass in gram of any substance is obtained from the relationship;
Mass= number of moles × molar mass
From the sequence of the reaction, the number of moles of Lithium diisopropylamide is 6.75mmol which is the same as 6.75 × 10^-3 moles
Molar mass of base= 107.1233 g/mol
Hence mass of the base is given by;
6.75 × 10^-3 moles × 107.1233 g/mol = 0.72 g
g What is the half-life for a particular reaction if the rate law is rate = (1291 M⁻¹*min⁻¹)[A]² and the initial concentration of A is 0.250 M?
Answer:
[tex]t_{1/2}=3.10x10^{-3}min=0.186s[/tex]
Explanation:
Hello,
In this case, for the calculation of the half-life for the mentioned reaction we first must realize that considering the units of the rate constant and the form of the rate law, it is a second-order reaction, therefore, the half-life expression is:
[tex]t_{1/2}=\frac{1}{k[A]_0}[/tex]
Therefore, we obtain:
[tex]t_{1/2}=\frac{1}{1291\frac{1}{M*min}*0.250M}\\\\t_{1/2}=3.10x10^{-3}min=0.186s[/tex]
Regards.
The half-life for the reaction is 0.003 mins
From the question given above, the following data were obtained:
Rate law = (1291 M⁻¹min⁻¹)[A]²
Initial concentration of A = 0.250 M
Half-life (t½) =?From the rate law given, we can see that the reaction is indicating a 2nd order reaction.
Thus, the half-life can be obtained as follow:
t½ = 1 / K[A₀]
t½ = 1 / (1291 × 0.25)
t½ = 0.003 minsTherefore, the half-life for the reaction is 0.003 mins
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What are the advantages of having proof before you make any conclusion about your own understanding for scientific method?
Answer:
Helps in accepting and defending the conclusion.
Explanation:
The main advantages of having proof before you make any conclusion is that it gives a reason for accepting the answer given by you because you have the proof to prove your answer so no one questions on your answer. The proof give you strength to defend your conclusion and make your conclusion right in front of the world. Without proof no one can accept your answer because every answer of a scientific question wants a proof for its validation.
How many bonding and antibonding molecular orbitals are there in methane, CH4?
Bonding orbitals Antibonding orbitals
Zero Zero
One One
Two Two
Three Three
Four Four
Answer:
Four Four
Explanation:
A molecule is formed by the overlap of orbitals. The combination of atomic orbitals during bond formation leads to the formation of bonding and anti bonding molecular orbitals.
When a molecule is formed, the number of bonding molecular orbitals must be equal to the number of anti bonding molecular orbitals.
Hence, when methane is formed, four bonding and four anti bonding orbitals are formed because methane forms four bonds per molecule.
-
What type of change, physical or chemical, takes place in each
of the following?
a. Pie dough is rolled into thin pieces for a crust.
b. A silver pin tarnishes in the air.
c. A tree is cut into boards at a saw mill.
d. Food is digested.
e. A chocolate bar melts.
Answer:
a. Physical Change
b. Chemical Change
c. Physical Change
d. Chemical Change
e. Physical Change
Physical and chemical change has been differentiated by the formation of new substances. Silver pin tarnishing and digestion of food are considered chemical changes. Thus, options b and d are correct.
What are physical and chemical changes?Chemical changes are characterized by alterations in the properties of the substances that results in the formation of new substances that differs in their composition and properties. These changes are said to be permanent changes that cannot be reversed back into their main constituents.
Physical changes are said to be temporary changes that are reversible as the substance produced has the same structures and includes changes in texture, color, pattern, temperature, state of matter, etc.
Silver tarnishes under air is a chemical change as it undergoes a chemical reaction under oxygen and produces a new product. Digestion of food is also a chemical change that breaks the food into smaller pieces under the action of the enzymes.
Rolling of the pie dough, cutting the trees into boards, and melting the chocolate bars are physical changes as no new substances with different chemical compositions are produced.
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A reaction between 7.0 g of copper(II) oxide and 50 mL of 0.20 M nitric acid produces
copper(II) nitrate, Cu(NO3)2 and water.
(c) Determine the limiting reactant.
(d) Calculate the mass of excess reactant after the reaction.
(ANS: 6.6068g)
(e) Determine the percentage yield if the actual mass of copper (II) nitrate obtained from
the reaction is 0.85 g.
(ANS: 90.64%)
How to get the mass of HNO3 from here? I only managed to get mass of NO3 based on the molarity formula. thanks!
Answer:
(c) Nitric acid [tex]\rm HNO_3\, (aq)[/tex] is the limiting reactant.
(d) Approximately [tex]6.6\; \rm g[/tex] of [tex]\rm CuO\, (s)[/tex] will be in excess.
(e) The percentage yield of [tex]\rm Cu(NO_3)_2[/tex] is approximately [tex]91\%[/tex]. (Rounded to two significant figures, as in other quantities in the question.)
Explanation:
Start with the balanced chemical equation:
[tex]\rm CuO\, (s) + 2\; HNO_3\, (aq) \to Cu(NO_3)_2\, (aq) + H_2O\, (l)[/tex].
Look up relevant relative atomic mass data on a modern periodic table:
[tex]\rm Cu[/tex]: [tex]63.546[/tex].[tex]\rm O[/tex]: [tex]\rm 15.999[/tex].[tex]\rm H[/tex]: [tex]1.008[/tex].[tex]\rm N[/tex]: [tex]14.007[/tex].Calculate the formula mass of the species:
[tex]M(\mathrm{CuO}) = 63.546 + 15.999 = 79.545\; \rm g\cdot mol^{-1}[/tex].[tex]M(\mathrm{Cu(NO_3)_2}) = 63.546 + 2\times (14.007 + 3 \times 15.999) = 187.554\; \rm g\cdot mol^{-1}[/tex].Limiting ReactantThere are two reactants in this reaction: [tex]\rm CuO[/tex] and [tex]\rm HNO_3\, (aq)[/tex]. Assume that [tex]\rm CuO\![/tex] is the limiting one. In other words, assume that all the [tex]\rm CuO\!\![/tex] is consumed before [tex]\rm HNO_3\, (aq)\![/tex] was.
Consider: how many moles of [tex]\rm HNO_3\, (aq)\!\![/tex] would be required to convert all that [tex]7.0\; \rm g[/tex] of [tex]\rm CuO\!\!\![/tex] to [tex]\rm Cu(NO_3)_2[/tex]?
Calculate the number of moles of [tex]\rm CuO[/tex] formula units in [tex]7.0\;\rm g[/tex] of
[tex]\displaystyle n({\rm CuO}) = \frac{m}{M} = \frac{7.0\; \rm g}{79.545\; \rm g \cdot mol^{-1}} \approx 0.088001\; \rm mol[/tex].
Note the ratio between the coefficients of [tex]\rm CuO\, (s)[/tex] and [tex]\rm HNO_3\, (aq)[/tex]:
[tex]\displaystyle \frac{n(\mathrm{HNO_3\, (aq)})}{n(\mathrm{CuO\, (s)})} = \frac{2}{1} = 2[/tex].
Therefore:
[tex]\begin{aligned}&n(\text{$\mathrm{HNO_3\, (aq)}$, consumed (under assumption)})\\ &= \frac{n(\text{$\mathrm{HNO_3\, (aq)}$, consumed})}{n(\mathrm{CuO\, (s)})}\cdot n(\mathrm{CuO\, (s)}) \\ &\approx 2 \times 0.088001\; \rm mol \approx 0.17600\; \rm mol\end{aligned}[/tex].
On the other hand, how many moles of [tex]\rm HNO_3\, (aq)[/tex] are actually available?
Convert the volume of that [tex]\rm HNO_3\, (aq)[/tex] solution to the standard unit (liter.)
[tex]V(\rm HNO_3\, (aq)) = 50\; \rm mL = 0.050\; \rm L[/tex].
Calculate the number of moles of [tex]\rm HNO_3\, (aq)[/tex] in that [tex]0.20\; \rm M[/tex] solution:
[tex]n({\rm HNO_3\, (aq)}) = c\cdot V = 0.050\; \rm L \times 0.20\; \rm mol \cdot L^{-1} = 0.010\; \rm mol[/tex].
Apparently, the quantity of [tex]\rm HNO_3\, (aq)[/tex] required exceeded the quantity that is available. Therefore, the assumption is invalid, and [tex]\rm CuO[/tex] cannot be the limiting reactant. At the same time,
Mass of the reactant in excessSince it is now known that all that [tex]0.010\; \rm mol[/tex] of [tex]\rm HNO_3\, (aq)[/tex] will be consumed, apply that coefficient ratio again to obtain the quantity of [tex]\rm CuO[/tex] consumed in this reaction:
[tex]\begin{aligned}&n(\text{$\mathrm{CuO}$, consumed})\\ &= n(\text{$\mathrm{HNO_3\, (aq)}$, consumed}) \left/\frac{n(\text{$\mathrm{HNO_3\, (aq)}$, consumed})}{n(\mathrm{CuO\, (s)})}\right. \\ &\approx (0.010 \; \rm mol) / 2 \approx 0.0050\; \rm mol\end{aligned}[/tex].
It was already shown that the formula mass of [tex]\rm CuO[/tex] is (approximately) [tex]79.545\; \rm g \cdot mol^{-1}[/tex]. Therefore, the mass of that [tex]0.0050\; \rm mol[/tex] formula units of [tex]\rm CuO\![/tex] would be:
[tex]\begin{aligned}& m(\text{$\rm CuO$, consumed}) \\&= n \cdot M \approx 0.0050\; \rm mol \times 79.545\; \rm g\cdot mol^{-1} \\&\approx 0.39773\; \rm g\end{aligned}[/tex].
Before the reaction, [tex]7.0\; \rm g[/tex] of [tex]\rm CuO[/tex] is available. Therefore, all that [tex]7.0\; \rm g - 0.39773\; \rm g \approx 6.6\; \rm g[/tex] of [tex]\rm CuO\![/tex] would be in excess.
Percentage YieldSimilarly:
[tex]\displaystyle \frac{n(\mathrm{HNO_3\, (aq)})}{n(\mathrm{Cu(NO_3)_2\, (aq}))} = \frac{2}{1} = 2[/tex].
Apply this ratio to find the theoretical yield of [tex]\rm Cu(NO_3)_2[/tex]:
[tex]n(\text{$\mathrm{Cu(NO_3)_2\, (aq)}$, theoretical yield}) \approx (0.010 \; \rm mol) / 2 \approx 0.0050\; \rm mol[/tex].
Find the mass of that [tex]0.0050\; \rm mol[/tex] of [tex]\rm Cu(NO_3)_2[/tex] formula units using its formula mass:
[tex]m(\text{$\rm Cu(NO_3)_2\, (aq)$, theoretical yield}) \approx 0.93777\; \rm g[/tex].
Calculate the percentage yield given that the actual yield is [tex]0.85\; \rm g[/tex]:
[tex]\begin{aligned}&\text{Percentage Yield} \\ &= \frac{\text{Actual Yield}}{\text{Theoretical Yield}}\times 100\% \\ &= \frac{0.85\; \rm g}{0.93777\; \rm g} \times 100\% \approx 0.91\% \end{aligned}[/tex].
(Rounded to two significant figures.)
(c) The limiting reactant is HNO₃
(d) The mass of the excess reactant after the reaction is approximately 6.6 grams
(e) The percentage yield of copper (II) nitrate from the reaction is approximately 90.64%
The reason the above values are the correct values is as follows;
The given parameters are;
The mass of copper(II)oxide in the reaction = 7.0 g
The volume of the 0.20 M nitric acid, HNO₃ = 50 mL
(c) Concentration of the reactants
The molar mass of CuO = 79.545 g/mol
Number of moles = Mass/(Molar mass)
The number of moles of CuO = (7 g)/79.545 g/mol ≈ 0.088 moles
50 mL of 0.20 M HNO₃, contains 50/1000 × 0.2 = 0.01 moles of HNO₃
The chemical equation for the reaction is CuO + 2HNO₃ → Cu(NO₃)₂ + H₂O
Therefore;
One mole of CuO reacts with two moles of HNO₃ to produce one mole of Cu(NO₃)₂ and one mole of H₂O
Therefore, 0.088 moles of CuO reacts with 2 × 0.088 = 0.176 moles of HNO₃
Given that there is only 0.01 moles of HNO₃, the limiting reactant is the HNO₃, which is not enough to completely react with the CuO which is the excess reactant
(d) The mass of the CuO that reacts with the 0.01 moles of HNO₃ is given as follows;
1 mole of CuO reacts with 2 moles HNO₃
0.01 moles of HNO₃ will react with 0.01/2 = 0.005 moles of CuO
Mass = Number of moles × Molar mass
The mass of 0.005 moles of CuO = 0.005 moles × 79.545 g/mol = 0.397725 grams
The mass of the CuO left = Initial mass - Reacting mass
∴ The mass of the CuO left = 7 grams - 0.397725 grams = 6.602275 grams
The mass of the excess reactant (CuO) after the reaction ≈ 6.6 grams
(e) The theoretical number of moles of copper (II) nitrate, Cu(NO₃)₂ produced = Half the number of moles of HNO₃ in the reaction
The number of moles of HNO₃ in the reaction = 0.01 moles
∴ The theoretical number of moles of copper (II) nitrate, Cu(NO₃)₂ produced = (1/2) × 0.01 moles = 0.005 moles
The molar mass of Cu(NO₃)₂ = 187.56 g/mol
The theoretical mass of Cu(NO₃)₂ produced = 0.005 moles × 187.56 g/mol = 0.9378 grams
The actual yield of copper (II) nitrate is 0.84 g
[tex]Percentage \ yield = \mathbf{\dfrac{Actual \ yield}{Theoretical \ yield} \times 100}[/tex]
Therefore;
[tex]\% \ yield \ of \ Cu(NO_3)_2 = \dfrac{0.85 \, g}{0.9378 \, g} \times 100 \approx 90.64 \%[/tex]
The percentage yield of copper (II) nitrate, %yield ≈ 90.64%
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A measurement of 9.15 is divided by another measurement of 16.23. What is the correct answer, taking into account appropriate significant digits?
Answer:
[tex]0.564[/tex]
Explanation:
Hello,
In this case, by performing the given division we obtain:
[tex]\frac{9.15}{16.23}=0.563770795[/tex]
Nevertheless since 9.15 has three significant figures and 16.23 four, we must show the result with three significant figures taking into account that it must be shown with the least significant figures from the initial data:
[tex]0.564[/tex]
Regards.