If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2?
1/2N2(g)+3/2H2(g)-->NH3(g)
a. 0.173 M/s
b. 0.345 M/s
c. 0.690 M/s
d. 245 M/s
e. 0.518 M/s
That'd be my choice.
idk im trynna knmow
To find the rate of disappearance of N2, we need to compare the stoichiometric coefficients of N2 and NH3 in the balanced chemical equation.
From the balanced equation, we can see that 1 mole of N2 reacts to form 2 moles of NH3.
Therefore, the rate of disappearance of N2 is half the rate of formation of NH3.
Given that the rate of formation of NH3 is 0.345 M/s, we can calculate the rate of disappearance of N2 by dividing the rate of formation by 2.
Rate of disappearance of N2 = (0.345 M/s) / 2 = 0.173 M/s
Therefore, the rate of disappearance of N2 is 0.173 M/s, which corresponds to option a.