The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of

Question

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×104 s1 at a certain temperature.

Part A What is the half-life for this reaction?

t1/2 = m s

Part B 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.

t = m s

Part C If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.74 M ? Express your answer using two significant figures.

t = m s

Part D If the initial concentration of SO2Cl2 is 0.175 M , what is the concentration of SO2Cl2 after 180 s ?

[SO2Cl2]t = m M

Part E If the initial concentration of SO2Cl2 is 0.175 M , what is the concentration of SO2Cl2 after 450 s ?

[SO2Cl2]t = m M

Explanation / Answer

A)

Half life time = 0.693/(1.44*10^(-4)) = 4812.5 sec

= 4812.5/60 = 80.21 min

B)

K = (1/t)ln(a/x)

1.44*10^(-4) = (1/t)ln(100/25)

t = 9627.05 sec

= 160.451 min

c)

1.44*10^(-4) = (1/t)ln(1/0.74)

t = 2091 sec

   = 34.85 min

d) 1.44*10^(-4) = (1/180)ln(0.175/x)

x = after 180 sec = 0.17 M

e)

1.44*10^(-4) = (1/450)ln(0.175/x)

x = after 450 sec = 0.164 M

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