At elevated temperatures, methylisonitrile (CH_3NC) isomerizes to acetonitrile (

Question

At elevated temperatures, methylisonitrile (CH_3NC) isomerizes to acetonitrile (CH_3CN): CH_3NC (g) rightarrow CH_3CN (g) At the start of an experiment, there are 0.200 mol of reactant and 0 mol of product in the reaction vessel. After 25 min, 0.121 mol of reactant (CH_3NC) remain. There are ________ mol of product (CH_3CN) in the reaction vessel. A) 0.200 B) 0.121 C) 0.079 D) 0.321 E) 0.022 What is the rate constant (in s^-1) of a first-order process that has a half-life of 503 s? A) 7.26 times 10^2 B) 1.99 times 10^-3 C) 3.49 times 10^2 D) 1.38 times 10^-3 The rate constant for a particular second-order reaction is 0.47 M^-1 s^-1. If the initial concentration of reactant is 0.25 mol/L, it takes __________ s for the concentration to decrease to 0.20 mol/L. A) 1.4 B) 0.20 C) 1.0 D) 2.1 E) 0.47 Given the following rate law, how does the rate of reaction change if the concentration of Y

Explanation / Answer

8) At elevated temperature-

CH3NC (g) ------> CH3CN (g)

At the start of the experiment, there are 0.200 mol of reactant (CH3NC) and 0 mol of product (CH3CN) in the reaction vessel.

After 25 min of reaction 0.121 moles of reactant remains and 0.079 moles of reactant has disappeared, so it must have turned into 0.079 moles of product.

C) 0.079 is correct option.

9) The relation between rate constant k and the half-life t1/2 of a first-order reaction-

t1/2 = ln2/k

t 1/2 = 0.693/k

k = 0.693/t1/2

k = 0.693/503 s

k = 0.001377

k = 1.38 x 10^-3 s^-1

D) 1.38 x 10^-3 s^-1 is correct option.

10)                                                                                                                                            

The rate constant for a particular second-order reaction is 0.47 M1s1 .

If the initial concentration A0 = 0.25 mol/L

The concentration A after time t = 0.20 mol/L

1/A -1/A0 = kt

1 / 0.20 - 1 / 0.25 =1M

1M = 0.47M-1s-1 t

t = 1 M/0.47M-1s-1

t = 2.13 s

D) 2.1 is correct option.

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