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Chemistry
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17 Nov 2019

Part A

The reaction between nitrogen dioxide and carbon monoxide is

NO2(g)+CO(g)→NO(g)+CO2(g)

The rate constant at 701 K is measured as 2.57 M−1⋠s−1 and that at 895 K is measured as 567 M−1⋠s−1. The activation energy is 1.5×102 kJ/mol.

Predict the rate constant at 525 K .

Express the rate constant in liters per mole-second to three significant figures.

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Irving Heathcote
Irving HeathcoteLv2
16 Sep 2019

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Related questions

2 things:

1. How did they flip 5.40=Ea/R(3.09x10^-4/K) to Ea=5.40 (K/3.09X10^-4)R

2: SOLVE 14.8!!!!

1) The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 ×10−10 s−1 at 25°C. Calculate the rate constant at 58.3°C if the activation energy is 116 kJ/mol.

(Enter your answer in scientific notation.)answer

2)Given the same reactant concentrations, the reaction

CO(g) + Cl2(g) → COCl2(g)at 259°C is 272 times as fast as the same reaction at 147°

C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.


kJ/mol answer

3)For a certain reaction, the frequency factor A is 7.5 ×109 s−1 and the activation energy is 24.5 kJ/mol.

What is the rate constant for the reaction at 92°C

(Enter your answer in scientific notation.) answer

4)The rate constant of a first-order reaction is 3.25 ×10−4 s−1 at 350.°C. If the activation energy is 107 kJ/mol,

calculate the temperature at which its rate constant is 9.85 ×10−4 s−1.

5)The rate at which tree crickets chirp is 1.80 ×102 per minute at 29°C but only 37.9 per minute at 6.5

°C. From these data, calculate the activation energy for the chirping process.

kJ/mol answer

6)Consider the following elementary step

X + 2Y →XY2

If the initial rate of formation of XY2 is 0.0076 M/s and the initial concentrations of X and Y are 0.38 Mand 0.64 M, what is the rate constant for the reaction?

M−2s−1 answer

7)The activation energy for the decomposition of hydrogen peroxide is 59.0 kJ/mol. When the reaction is catalyzed by the enzyme catalase, it is 6.00 kJ/mol.

2H2O2(aq) →2H2O(l) + O2(g)


Calculate the temperature that would cause the nonenzymatic catalysis to proceed as rapidly as the enzyme-catalyzed decomposition at 20.0°C. Assume the frequency factor, A, to be the same in both cases. Report your answer to 3 significant figures.

8)The activation energy (Ea) for the reaction

2N2O(g) → 2N2(g) + O2(g) ΔH

o
= −164 kJ/mol


is 370.0 kJ/mol. What is the (Ea) for the reverse reaction?

kJ/mol answer


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