Rate = -?[NOBr]/?t = k[NOBr]^22 NOBr(g) - 2 NO(g) + Br2(g)a) If the half-life for this reaction is 2.00 s when [NOBr]0 =0.900 M, calculate the value of k for this reaction.I calculated this to be 0.556 L/mol*sb) How much time (in seconds) is required for the concentration ofNOBr to decrease to 0.144 M?This part is driving me crazy. I've done a ton of sample problemsand gone through the answers to similar questions on here, but Ikeep getting the wrong answer. Please help?

Question

Rate = -?[NOBr]/?t = k[NOBr]^22 NOBr(g) -> 2 NO(g) + Br2(g)a) If the half-life for this reaction is 2.00 s when [NOBr]0 =0.900 M, calculate the value of k for this reaction.I calculated this to be 0.556 L/mol*sb) How much time (in seconds) is required for the concentration ofNOBr to decrease to 0.144 M?This part is driving me crazy. I've done a ton of sample problemsand gone through the answers to similar questions on here, but Ikeep getting the wrong answer. Please help?

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