The rate constant for a certain reaction is k = 9.00 * 10^-3s^-1 . If the initia

Question

The rate constant for a certain reaction is k = 9.00 * 10^-3s^-1 . If the initial reactant concentration was 0.450 M, what will the concentration be after 2.00 minutes?

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 148 Times 10-s-l at a certain temperature What is the half-life for this reaction'? How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? Express your answer using two significant figures. If the initial concentration of SO2Cl2 is 1 00 M how long will it take for the concentration to decrease to 0 80M? Express your answer using two significant figures. If the initial concentration of SO2 Cl2 is 0 175M what is the concentration of SO2Cl2 after 200s? If the initial concentration of SO2 Cl2 is 0 175M what is the concentration of SO2Cl2 after 500s?

Explanation / Answer

k = 9.00 * 10^-3s^-10

now, this is a first order reaction because the unit of rate constant is s-1

thus, the governing equation is :-

k*t = ln{[A0]/[A]} , where t = time = 2 minutes = 120 seconds ; [A0] = initial concentration = 0.45 M and [A] = concentration after time 't'

thus,

or, (9*10-3)*120 = ln{(0.45)/[A]}

or, [A] = 0.153 M

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