Question

A chemistry graduate student is studying the rate of this reaction:

NH4OH(aq)→NH3(aq)+H2O(aq)
She fills a reaction vessel with and measures its concentration as the reaction
proceeds: time (seconds).
1. Write the rate law for this reaction.
2. Calculate the value of the rate constant.

Answer 1

The rate law for the reaction is first order concerning NH4OH, and the rate constant is 1.0 h^-1.

Step-by-step explanation:

The rate law for the given reaction can be determined by analyzing the relationship between the concentrations of the reactants and the rate of the reaction. Based on the provided data, the rate law for the reaction NH4OH(aq) → NH3(aq) + H2O(aq) is first order concerning NH4OH. This means that the rate of the reaction is directly proportional to the concentration of NH4OH.

To calculate the value of the rate constant, we can choose any of the given data points and substitute the values into the rate law equation. Let's use the second data point:

Rate = k[NH4OH]

Rate = (2.0 × 10^-3 mol L^-1 h^-1) = k(2.0 × 10^-3 M)

Solving for k:

k = (2.0 × 10^-3 mol L^-1 h^-1) / (2.0 × 10^-3 M) = 1.0 h^-1

Therefore, the rate constant for this reaction is 1.0 h^-1.

Answer 2

See explaination

Step-by-step explanation:

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