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November 23, 2014

November 23, 2014

Posted by **Kyo** on Monday, May 17, 2010 at 12:19am.

Okay so, I tried using Graham's law for this problem. Rate A was 4.73. Molar Mass of bromine was 79.904 and the molar mass of gas B, CH4, is 16.04246. I plugged everything in and got 10.6 minutes for the rate of effusion for CH4 gas, but the answer is 1.5 minutes. Please tell me what I did wrong?

- Chemistry -
**DrBob222**, Monday, May 17, 2010 at 1:43pmI can't duplicate your numbers although I tried several combinations; however, you have made at least two errors.

a)Error #1 is that you are calling rate the same as time. It isn't. The time it takes the gas to go through is obvious, the rate is the AMOUNT (such as 1 L) per time. Therefore, the rate for Br2 is 1 L/4.73 min. (The problem doesn't mention volume nor does it say the volume is the same for both gases but I assume it is.

b)Error #2 is that you have used the molar mass of Br as 79.9 but it is twice that or 159.8.

rate 1/rate 2 = sqrt(M2/M1)

rate 1 = rate Br2 = 1/4.73 min

rate 2 = rate CH4 = 1/x min

M1 = molar mass Br2 = 159.8

M2 = molar mass CH4 = 16

1/4.73/1/x = sqrt(16/159.8)

0.2114/1/x = 0.3164

0.2114 = 0.3164*(1/x)

(1/x) = 0.2114/0.3164 = 0.668 and

x = 1/0.668 = 1.496 min which rounds to 1.5 min which is the TIME it takes for CH4 to effuse under the same conditions, not the rate at which it does so.

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