#### Question

A first order reaction takes 40 minutes for 30% decomposition. Calculate t_{1/2} for this reaction. (Given log 1.428 = 0.1548)

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The experimental data for decomposition of N_{2}O_{5}

[`2N_2O_5 -> 4NO_2 + O_2`] in gas phase at 318K are given below:

t(s |
0 | 400 | 800 | 1200 | 1600 | 2000 | 2400 | 2800 | 3200 |

`10^2xx[N_2O_5]mol L^(-1)` | 1.63 | 1.36 | 1.14 | 0.93 | 0.78 | 0.64 | 0.53 | 0.43 | 0.35 |

**(i) **Plot [N_{2}O_{5}] against *t*.

**(ii) **Find the half-life period for the reaction.

**(iii)** Draw a graph between log [N_{2}O_{5}] and *t.*

**(iv) **What is the rate law?

**(v) **Calculate the rate constant.

**(vi) **Calculate the half-life period from *k *and compare it with (ii).

#### Reference Material

Solution for question: A First Order Reaction Takes 40 Minutes for 30% Decomposition. Calculate t1/2 for this Reaction. concept: Integrated Rate Equations - Half-life of a Reaction. For the courses CBSE (Arts), CBSE (Commerce), CBSE (Science), HSC Science (Computer Science), HSC Science (Electronics), HSC Science (General) , PUC Karnataka Science