The average rate of the following reaction at a certain temperature is 1.42×10 -

Question

The average rate of the following reaction at a certain temperature is 1.42×10-2 M/min. Calculate the value for the rate of change of [NH4Cl], in M/min, at this temperature. Report your answer to three significant figures in scientific notation.


AgNO3(aq) + NH4Cl(aq) AgCl(s) + NH4NO3(aq)

If the intial concentration of AgNO3 is 0.548 M and the initial concentration of NH4Cl is 0.109 M, determine the concentration of AgNO3 (in M) after 39 seconds. Assume the volume of the solution does not change and report your answer to three significant figures in scientific notation.

Explanation / Answer

Rate = -d[AgNO3]/dt
1.42*10^-2 = -(x-0.548)/(39*1/60)
final [AgNO3] = 0.5387 M = 0.539 M
Rate = -d[NH4Cl]/dt
1.42*10^-2 = -(x-0.109)/(39*1/60)
final [NH4Cl] = 0.09977 M = 0.998 M

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