At a certain temperature the rate of this reaction is first order in NH₂OH with a rate constant of 1.23 s¹:NH₂OH(aq) → NH3(aq) + H₂O (aq)Suppose a vessel contains NH4OH at a concentration of 0.160 M. Calculate the concentration of NH4OH in the vessel 0.940 seconds later. You may assume noother reaction is important.Round your answer to 2 significant digits.x10XŚ

Answered: At a certain temperature the rate of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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At a certain temperature the rate of this reaction is first order in NH₂OH with a rate constant of 1.23 s¹:
NH₂OH(aq) → NH3(aq) + H₂O (aq)
Suppose a vessel contains NH4OH at a concentration of 0.160 M. Calculate the concentration of NH4OH in the vessel 0.940 seconds later. You may assume no
other reaction is important.
Round your answer to 2 significant digits.
x10
X
Ś

Expert Solution

Step 1: Introduction

Given the rate of reaction is first order and for the first order reaction, formula for calculating the concentration of reactant after time t, having its initial concentration and time passed with rate constant value is:

k × t = ln(A_°/A_t)

Where A_°= initial reactant concentration

A_t = reactant concentration after time 't' ,

t= time used ,

k = rate constant value

Given, rate constant, k = 1.23 s^-1

A_o = 0.160 M

t = 0.940 sec

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