1
answer
0
watching
210
views
28 Sep 2019
Rate = -?[NOBr]/?t = k[NOBr]^2
2 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*s
b) 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?
Rate = -?[NOBr]/?t = k[NOBr]^2
2 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*s
b) 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?
2 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*s
b) 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?
Tod ThielLv2
29 Sep 2019