Question

The first-order reaction, 2 N2O(g) → 2 N2(g) + O2(g), has a rate constant equal to 0.76 s-1 at 1000 K. How long will it take for the concentration of N2O to decrease to 6.0% of its initial concentration? 3.7 s 13 s 0.27 s 17 s

Answer 1

It will take approximately 3.7 seconds for the concentration of N2O to decrease to 6.0% of its initial concentration.

Step-by-step explanation:

To determine how long it will take for the concentration of N2O to decrease to 6.0% of its initial concentration, we need to use the integrated rate law for a first-order reaction. The integrated rate law for a first-order reaction is given by: ln(N2O) = -kt + ln(N2O0), where N2O is the concentration at time t, k is the rate constant, and N2O0 is the initial concentration.

Plugging in the given values, we get: ln(0.06) = -0.76t + ln(1.0), where t is the time in seconds. Solving for t, we get t ≈ 3.7 seconds.

Answer 2

t=3.7 sec this much time it will take

Step-by-step explanation:

first order: the reaction in which rate depends only on one ractanta and depend linearly.

As given the question that reaction is first order so we will use first order kinetic equation.

Assume that initial concentration is a

then the final concentration is 0.06a

`Kt=ln(a)/(0.06a)`

`k=0.76s^(-1)`

after calculation

t=3.7 sec