The rate law for a reaction is determined by the reaction's mechanism, but it can also be approximated experimentally using the concentrations of the reactants and the order of the reaction.

In this case, we are given that the reaction is: NH4OH(aq) + NH3(aq) - H2O(aq)

Assuming the reaction is first order with respect to NH4OH, the rate law would be: rate = k[NH4OH]

To find the rate constant k, we can use the formula for a first order reaction: ln([A]0/[A]t) = kt

Where:
[A]0 is the initial concentration of NH4OH
[A]t is the concentration of NH4OH at time t
k is the rate constant
t is the time

Let's use the data from time 0 to time 1.0 seconds:

ln([A]0/[A]t) = ln(0.400M/0.277M) = 0.36

So, 0.36 = k(1.0 s)

Solving for k gives k = 0.36 / 1.0 s = 0.36 s^-1

Rounding to two significant figures, k = 0.36 s^-1.

Question

The rate law for a reaction is determined by the reaction's mechanism, but it can also be approximated experimentally using the concentrations of the reactants and the order of the reaction.

In this case, we are given that the reaction is: NH4OH(aq) + NH3(aq) -> H2O(aq)

Assuming the reaction is first order with respect to NH4OH, the rate law would be: rate = k[NH4OH]

To find the rate constant k, we can use the formula for a first order reaction: ln([A]0/[A]t) = kt

Where:
[A]0 is the initial concentration of NH4OH
[A]t is the concentration of NH4OH at time t
k is the rate constant
t is the time

Let's use the data from time 0 to time 1.0 seconds:

ln([A]0/[A]t) = ln(0.400M/0.277M) = 0.36

So, 0.36 = k(1.0 s)

Solving for k gives k = 0.36 / 1.0 s = 0.36 s^-1

Rounding to two significant figures, k = 0.36 s^-1.

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