Question

The decomposition of hydrogen peroxide, H2O2, is first order with a rate constant, k = 3.66×10^-3 s^-1. If the initial concentration of H2O2 is 1.05 M, calculate [H2O2] after 187 s. A) 0.978 B) 0.234 C) 0.863 D) 0.203 E) 0.530

Name: the decomposition of hydrogen peroxideh2o2 is first order with a rate constantk 36610 3 s 1 if the initial concentration ofh2o2 is 105 m calculate h2o2 after 187 s a 0978 b 0234 c 0863 d 020 74208
Uploaded: 2022-05-25T09:09:26-08:00
Duration: 4 min 52 s
Channel: Preeti Kumari
Description: the decomposition of hydrogen peroxideh2o2 is first order with a rate constantk 36610 3 s 1 if the initial concentration ofh2o2 is 105 m calculate h2o2 after 187 s a 0978 b 0234 c 0863 d 020 74208

          The decomposition of hydrogen peroxide, H2O2, is first order with a rate constant, k = 3.66×10^-3 s^-1. If the initial concentration of H2O2 is 1.05 M, calculate [H2O2] after 187 s.
A) 0.978 B) 0.234 C) 0.863 D) 0.203 E) 0.530

Added by Joseph K.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Preeti Kumari

05/25/2022

Step 1

05 / [H2O2]) using the given rate constant and time: \[3.66 \times 10^{-3} \text{ s}^{-1} \times 187 \text{ s} = \ln(1.05 / [H2O2])\] Show more…

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The decomposition of hydrogen peroxide, H2O2, is first order with a rate constant, k = 3.66×10^-3 s^-1. If the initial concentration of H2O2 is 1.05 M, calculate [H2O2] after 187 s. A) 0.978 B) 0.234 C) 0.863 D) 0.203 E) 0.530