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a)Assume the reaction 2Fe3+ + Sn2+ -> 2Fe2+ + Sn4+ has a ratelaw v = k[Fe3+][Sn2+]. If Fe2+ is produced at a rate of 0.12 molL-1 s-1 when the reactant concentrations are 0.30 mol L-1 for Fe3+,and 0.40 mol L-1 for Sn2+, then what is the value of the rateconstant, k ? Quote your answer to 2 decimal places.

Answer L.mol-1.s-1

b)

The half-life for the decomposition of a gaseous sample ofthioketene, H₂C=C=S at 500 Pa is 42 s. When thethioketene pressure is 250 Pa the half-life is 21 s. Determine theorder of the reaction, entering your answer as a number.

c)

At 1100 K, acetic acid decomposes via 2 competing, first orderreactions:

CH₃COOH -> CH₄ +CO₂,   k₁ = 3.4s^-1

CH₃COOH -> CH₂=C=O + H₂O,   k₂ = ? s^-1

The half life of acetic acid at this temperature is 0.10 s. Whatis the value of the rate constant, k₂?

d)

At 1100 K, acetic acid decomposes via 2 competing, first orderreactions:

CH₃COOH -> CH₄ +CO₂,   k₁ = 4.1s^-1

CH₃COOH -> CH₂=C=O + H₂O,   k₂ = ? s^-1

At 1100K, the yield of ketene (CH₂=C=O) is 71.5%.Estimate the rate constant, k₂, for the secondreaction

e)

The following mechanism has been proposed for recombination ofiodine atoms:

I + I -> I₂*, k₁ = [k1].0

I₂* -> I + I, k_-1 =[k-1].0

I₂* + M -> I₂, k₂ =[k2]

What is overall rate constant if k₁ = 4,k_-1 = 4 and k₂ = 0.04?

f)

The following mechanism has been proposed for recombination ofiodine atoms:

I + I -> I₂*, k₁ = 9.0

I₂* -> I + I, k_-1 = 5.0

I₂* + M -> I₂, k₂ =0.04

What is overall rate constant?

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