12.3 Rate laws  (Page 5/10)

How will each of the following affect the rate of the reaction: $\text{CO(}g)+{\text{NO}}_2(g)⟶{\text{CO}}_2(g)+\text{NO(}g)$ if the rate law for the reaction is $\text{rate}=k\left[{\text{NO}}_2\right]\left[\text{CO}\right]$ ?

(a) Increasing the pressure of NO ₂ from 0.1 atm to 0.3 atm

(b) Increasing the concentration of CO from 0.02 M to 0.06 M .

Regular flights of supersonic aircraft in the stratosphere are of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction $\text{NO}+{\text{O}}_3⟶{\text{NO}}_2+{\text{O}}_2$ is first order with respect to both NO and O ₃ with a rate constant of 2.20 $\times$ 10 ⁷ L/mol/s. What is the instantaneous rate of disappearance of NO when [NO] = 3.3 $\times$ 10 ⁻⁶ M and [O ₃ ] = 5.9 $\times$ 10 ⁻⁷ M ?

Radioactive phosphorus is used in the study of biochemical reaction mechanisms because phosphorus atoms are components of many biochemical molecules. The location of the phosphorus (and the location of the molecule it is bound in) can be detected from the electrons (beta particles) it produces:
${}_{\text{15}}^{\text{32}}\text{P}⟶{}_{16}^{32}\text{S}+{\text{e}}^{-}$
Rate = 4.85 $\times$ 10 ⁻² ${\text{day}}^{-1}\left[{}^{32}\text{P}\right]$

What is the instantaneous rate of production of electrons in a sample with a phosphorus concentration of 0.0033 M ?

The rate constant for the radioactive decay of ¹⁴ C is 1.21 $\times$ 10 ⁻⁴ year ⁻¹ . The products of the decay are nitrogen atoms and electrons (beta particles):
${}_{14}^6\text{C}⟶{}_{14}^6\text{N}+{\text{e}}^{-}$
$\text{rate}=k\left[{}_{14}^6\text{C}\right]$

What is the instantaneous rate of production of N atoms in a sample with a carbon-14 content of 6.5 $\times$ 10 ⁻⁹ M ?

The decomposition of acetaldehyde is a second order reaction with a rate constant of 4.71 $\times$ 10 ⁻⁸ L/mol/s. What is the instantaneous rate of decomposition of acetaldehyde in a solution with a concentration of 5.55 $\times$ 10 ⁻⁴ M ?

Alcohol is removed from the bloodstream by a series of metabolic reactions. The first reaction produces acetaldehyde; then other products are formed. The following data have been determined for the rate at which alcohol is removed from the blood of an average male, although individual rates can vary by 25–30%. Women metabolize alcohol a little more slowly than men:

Determine the rate equation, the rate constant, and the overall order for this reaction.

Under certain conditions the decomposition of ammonia on a metal surface gives the following data:

Determine the rate equation, the rate constant, and the overall order for this reaction.

Nitrosyl chloride, NOCl, decomposes to NO and Cl ₂ .
$\text{2NOCl(}g)⟶\text{2NO(}g)+{\text{Cl}}_2(g)$

Determine the rate equation, the rate constant, and the overall order for this reaction from the following data:

From the following data, determine the rate equation, the rate constant, and the order with respect to A for the reaction $A⟶2C.$

Nitrogen(II) oxide reacts with chlorine according to the equation:
$\text{2NO(}g)+{\text{Cl}}_2(g)⟶\text{2NOCl(}g)$

The following initial rates of reaction have been observed for certain reactant concentrations:

What is the rate equation that describes the rate’s dependence on the concentrations of NO and Cl ₂ ? What is the rate constant? What are the orders with respect to each reactant?

Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: ${\text{H}}_2(g)+\text{2NO(}g)⟶{\text{N}}_2\text{O(}g)+{\text{H}}_2\text{O(}g)$

Determine the rate equation, the rate constant, and the orders with respect to each reactant from the following data:

For the reaction $A⟶B+C,$ the following data were obtained at 30 °C:

(a) What is the order of the reaction with respect to [ A ], and what is the rate equation?

(b) What is the rate constant?

For the reaction $Q⟶W+X,$ the following data were obtained at 30 °C:

(a) What is the order of the reaction with respect to [ Q ], and what is the rate equation?

(b) What is the rate constant?

The rate constant for the first-order decomposition at 45 °C of dinitrogen pentoxide, N ₂ O ₅ , dissolved in chloroform, CHCl ₃ , is 6.2 $\times$ 10 ⁻⁴ min ⁻¹ .
${\text{2N}}_2{\text{O}}_5⟶{\text{4NO}}_2+{\text{O}}_2$

What is the rate of the reaction when [N ₂ O ₅ ] = 0.40 M ?

The annual production of HNO ₃ in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel.

(a) ${\text{4NH}}_3(g)+{\text{5O}}_2(g)⟶\text{4NO(}g)+{\text{6H}}_2\text{O(}g)$

(b) $\text{2NO(}g)+{\text{O}}_2(g)⟶{\text{2NO}}_2(g)$

(c) ${\text{3NO}}_2(g)+{\text{H}}_2\text{O(}l)⟶{\text{2HNO}}_3(aq)+\text{NO(}g)$

The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in O ₂ , what is the rate of formation of NO ₂ when the oxygen concentration is 0.50 M and the nitric oxide concentration is 0.75 M ? The rate constant for the reaction is 5.8 $\times$ 10 ⁻⁶ L ² /mol ² /s.

The following data have been determined for the reaction:
${\text{I}}^{\text{−}}+{\text{OCl}}^{\text{−}}⟶{\text{IO}}^{\text{−}}+{\text{Cl}}^{\text{−}}$

Determine the rate equation and the rate constant for this reaction.