I need help with these Kinetics questions, I've looked everywhere and I still havent been able to find the answers:
The decomposition reaction, X --> products, is zeroth-order with rate constant k=0.0921 mol L-1 s-1. How long will it take for the decomposition to be 25% complete, if the initial concentration of X is 1.35 mol/L?
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The reaction X + Y --> products was studied using the method of initial rates. The initial rate of consumption of X was measured in three different experiments. Data are provided below.
The first column: Expt #
Second column: [X] o (in mol/L)
Third column: [Y] o(in mol/L)
Last column: Initial Rate (in mol L -1 s - 1 )
1 0.200 0.200 1.310
2 0.600 0.200 0.4367
3 0.200 0.500 8.188
What is the value of the rate constant, k? (Use concentrations in mol/L and time in seconds. Enter your answer accurate to three significant figures.)
Hint: First determine the rate law, and then evaluate k.
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Thanks for the help in advance!