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2 years ago

Onsider the following elementary reaction:

Chemistry

1 answer:

Brilliant_brown [7]2 years ago

3 0

Answer:

$C_{O_2}=\frac{k_2C_{NO_2}C_{O}}{k_1C_{NO}}$

Explanation:

Hello,

In this case, for the given elementary reaction, the rate law takes the form:

$r=-k_1C_{NO}C_{O_2}+k_2C_{NO_2}C_{O}$

Nevertheless, at equilibrium, the rate becomes zero:

$0=-k_1C_{NO}C_{O_2}+k_2C_{NO_2}C_{O}$

Thus, we can solve for the concentration of O₂ in terms of the rate constants as shown below:

$k_1C_{NO}C_{O_2}=k_2C_{NO_2}C_{O}\\\\C_{O_2}=\frac{k_2C_{NO_2}C_{O}}{k_1C_{NO}}$

Best regards.

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3 years ago

1. Calculate the momentum of a 1,500 kg car traveling at 6 m/s.

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1. $9000kgm/s$

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3 years ago

If the chemist mistakenly makes 250 mL of solution instead of the 200 mL, what molar concentration of sodium nitrate will the ch

Evgesh-ka [11]

Answer:

0.120M is the concentration of the solution

Explanation:

Assuming the mass of sodium nitrate dissolved was 2.552g

Molar concentration is an unit of concentration widely used in chemsitry defined as the moles of solute (In this case NaNO3) in 1L of solution.

To find this question we must find the moles of NaNO3 in 2.552g. With this mass and the volume (250mL = 0.250L) we can find molar concentration as follows:

Moles NaNO3 -Molar mass: 84.99g/mol-

2.552g * (1mol / 84.99g) = 0.0300 moles NaNO3

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3 years ago

Consider the balanced equation for the following reaction:

Bad White [126]

Answer: The theoretical yield of the lithium chlorate is 1054.67 grams

Explanation:

To calculate the mass for given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Actual moles of lithium chlorate = 9.45 moles

Molar mass of lithium chlorate = 90.4 g/mol

Putting values in above equation, we get:

$9.45mol=\frac{\text{Actual yield of lithium chlorate}}{90.4g/mol}\\\\\text{Actual yield of lithium chlorate}=(9.45mol\times 90.4g/mol)=854.28g$

To calculate the theoretical yield of lithium chlorate, we use the equation:

$\%\text{ yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\times 100$

Actual yield of lithium chlorate = 854.28 g

Percentage yield of lithium chlorate = 81.0 %

Putting values in above equation, we get:

$81=\frac{854.28g}{\text{Theoretical yield of lithium chlorate}}\times 100\\\\\text{Theoretical yield of lithium chlorate}=\frac{854.28\times 100}{81}=1054.67g$

Hence, the theoretical yield of the lithium chlorate is 1054.67 grams

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2 years ago