101k views
0 votes
PLS HELP ITS DUE IN 10 MINS! how many grams of nitrogen gas is required to completely react with 14.2g of H2 at STP??

User Skalee
by
7.7k points

1 Answer

3 votes

To answer this question, we can use the balanced chemical equation for the reaction between hydrogen gas (H2) and nitrogen gas (N2) to form ammonia (NH3):

N2 + 3H2 → 2NH3

From the balanced equation, we can see that 3 moles of hydrogen gas are required to react with 1 mole of nitrogen gas to form 2 moles of ammonia.

First, we need to calculate the number of moles of hydrogen gas we have:

n(H2) = m/M = 14.2 g / 2.016 g/mol = 7.05 mol

Next, we can use the mole ratio between hydrogen and nitrogen from the balanced equation to calculate the number of moles of nitrogen gas required:

n(N2) = n(H2) / 3 = 7.05 mol / 3 = 2.35 mol

Finally, we can use the molar mass of nitrogen gas to convert from moles to grams:

m(N2) = n(N2) x M(N2) = 2.35 mol x 28.02 g/mol = 65.9 g

Therefore, 65.9 grams of nitrogen gas is required to completely react with 14.2 grams of hydrogen gas at STP.

Hope this Helps!

User Yaroslav Skachkov
by
8.0k points

No related questions found

Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.