Homework Help: Chemistry

Posted by Hannah on Sunday, February 19, 2012 at 6:14pm.

1. Nitric oxide reacts with bromine gas at elevated temperatures according to the equation,
2 NO(g) + Br2(g) = 2 NOBr(g)

The experimental rate law is rate = k[NO][Br2]. In a certain reaction mixture the rate of formation of NOBr(g) was found to be 4.50 x 10-4 mol L-l s-l. What is the rate of consumption of Br2(g), also in mol L-l s-l?

I think that the answer is 9.00 X e-4 because I multiplied 4.50 by 2.

Is this correct?

Chemistry - JSJFJF, Sunday, February 19, 2012 at 6:40pm
Yes it is.
Chemistry - Hannah, Sunday, February 19, 2012 at 7:57pm
thank you!
Chemistry - Rick, Monday, February 20, 2012 at 7:38pm
Wouldn't you divide it by 2?

4.50 NOBr x 1Br/2NOBR = 2.25BR

The NOBr cancel. Is this not correct

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