Asked by Ashley
1. For the simple decomposition reaction below, rate = k[AB]2 and k = 0.40 L/mols.
AB(g) A(g) + B(g)
If the initial concentration of AB is 1.60 M, what is [AB] after 13.0 s?
ANSWER:
(.4)(13)=5.2
1/1.6=.625
5.2-.625=4.575
1/4.575= .2185
I tried .22 & .21. They are both wrong. I have one try left. :( Please help me.
AB(g) A(g) + B(g)
If the initial concentration of AB is 1.60 M, what is [AB] after 13.0 s?
ANSWER:
(.4)(13)=5.2
1/1.6=.625
5.2-.625=4.575
1/4.575= .2185
I tried .22 & .21. They are both wrong. I have one try left. :( Please help me.
Answers
Answered by
DrBob222
I don't think the right answer is listed.
I think it should be 1/(5.2+0.625) = ??
I think the answer that is supposed to be correct is the 1/4.575; however, that is the same as the third one but the reciprocal has not been taken for the number. I don't think 0.2185 is correct.
I think it should be 1/(5.2+0.625) = ??
I think the answer that is supposed to be correct is the 1/4.575; however, that is the same as the third one but the reciprocal has not been taken for the number. I don't think 0.2185 is correct.
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