Please tell me the correct answer showing full explanation inorder to earn 10 pts and 5 stars)?

Question

Consider the following reaction:

N2(g) + 3H2 (g) →2NH3(g)

If the rate of formation of NH3 is 4.0 * 10^-4 mol/s, Then the rate of consumption of H2 is

a)2.0 * 10^-4 mol/s

b)4.0 *10^-4 mol/s

c)6.0 *10^-4 mol/s

d)1.2 *10^-3 mol/s

Kindly tell me the correct answer and show explanation. I promice to give 10 pts and 5 stars for the best answer.

Answer 1

For every 2 moles of NH3, 3 moles of H2 are consumed. So H2's rate will be 3/2 (or 1.5 times) greater than NH3's. So all you would have to do is multiply NH3's rate by 3/2 (1.5).

4 X (3/2) = 6

or 4 X 1.5 = 6.

So the answer is c!

[note: I realize I didn't include the 10^-4, but it's not necessary since most of the answer choices have the same exponent (-4). It would be necessary to include it in your calculations if the answer choices had different exponents.]

Answer 2

H2 consumed at 3/2 for every NH3 produced; therefore

3/2 * 4 x 10^-4 = ?

Should be 6 -----?