# stoichiometry

6mols of N2 are mixed with 12mol H2, according to the following equation.

N2+3H2----> 2NH3

a) which is the limiting reactant?

B) which chemical is in excess?

c) how many moles of excess reactant is left over?

d) how many moles of NH3 can be produced?

e)if only 6.4 mols of NH3 are produced What is the percent yield?

1. 👍 0
2. 👎 0
3. 👁 193
1. first, make sure the equation is balanced,,
to determine which is limiting, we calculate the amount of product produced by each given:
for 6 mol N2:
6 mol N2 * (2 mol NH3 / 1 mol N2) = 12 mol NH3
for 12 mol H2:
12 mol H2 * (2 mol NH3 / 3 mol H2) = 8 mol NH3

(a) since H2 produced less moles of NH3, H2 is limiting.

(b) thus N2 is in excess.

(c) we get the moles of N2 needed by the given amount of H2:
12 mol H2 * (1 mol N2 / 3 mol H2) = 4 mol N2
6 - 4 = 2 mol N2 left

(d) we already solved this in part (a) ,, the answer we got is 8 mol NH3

(e) percent yield = (actual yield)/(theoretical yield) * 100
percent yield = 6.4 / 8 * 100 = 80%

hope this helps~ :)

1. 👍 0
2. 👎 0

## Similar Questions

1. ### chemistry

Calculate the delta H for the reaction N2H4(l)+ O2(g) --> N2(g) + 2H20(l) Given the following data: 2NH3(g) + 3N20(g) --> 4N2(g) + 3H20(l) N20(g) + 3H2(g) --> N2H4(l) + H20(l) 2NH3(g) + 1/2O2(g) --> N2H4(l) + H20(l) H2(g) +

2. ### Chemistry

Calculate Delta H for 4NH3 + 5O2 --> 4NO + 6H2O using: N2 +O2 --> 2NO DH= -180.5 kJ N2 + 3H2 --> 2NH3 DH= -91.8 kJ 2H2 + O2 --> 2H2O DH= -483.6 kJ

3. ### chemistry

9. The reaction of 50 mL of N2 gas with 150 mL H2 gas to form ammonia via the equation: N 2(g) + 3H2 (g) → 2NH3 (g) will produce a total of mL of ammonia if pressure and temperature are kept constant

4. ### Chemistry

Calculate Delta H for the reaction CH4(g)+NH3(g)-->HCN(g)+3H2(g) given, N2(g)+3H2(g)->2NH3(g) DeltaH=-91.8kj C(s)+2H2(g)->CH3(g) DeltaH=-74.9kj h2(g)+2C(s)+N2(g)->2HCN(g) DeltaH=270.3kj

1. ### Chemistry

N2(g) + 3H2(g)  2NH3(g) at STP How many litres of ammonia gas is produced using 5 litres of H2? N2 + 3H2 ---> 2NH3 - the ratio between H2 and NH3 is 3 : 2 - it's given 5 litres of H2, so the volume of NH3 formed is 5/3*2 = 10/3

2. ### Chemistry

1. How many moles of ammonia NH3 are produced when 0.45 moles of nitrogen N2 reacts? N2 + 3H2 yields 2NH3 2. How many mililiters of water will be produced when 2.05 g of hydrogen reacts? The density of water is 1.00 g/mL ? 2H2 +

3. ### Chemistry

2n+3h2 gives 2nh3 find out the total number of molecules and atoms

4. ### Chemistry

Given the following equation: N2(g) + 3H2(g) = 2NH3(g). Determine to one decimal place the molar mass of each term, and WRITE EACH ONE AS A CONVERSION from moles to grams.

1. ### Chemistry

Calculate the value of Keq for the following equation. Heat + N2(g) + 3H2(g) ↔ 2NH3(g) [N2] = .533M [H2] = 1.600M [NH3] = 0.933M Bob if you're here, can you tell me if adding a substance like "Heat" to the equation changes the

2. ### Chemistry

The Kp for the following equilibrium system is 4.31 x 10‒4 at 375°C : N2(g) + 3H2(g) ↔ 2NH3(g). If 0.862 atm of N2 and 0.373 atm of H2 were mixed in a constant-volume flask and heated to 375°C, which of the following would

3. ### physical science

nitrogen and hydrogen react to form ammonia as follows N2(g)+3H2(g) -2NH3(g)

4. ### stoichiometry

6mols of N2 are mixed with 12mol H2, according to the following equation. N2+3H2----> 2NH3 a) which is the limiting reactant? B) which chemical is in excess? c) how many moles of excess reactant is left over? d) how many moles of