Question

Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How...

Consider the following balanced reaction between hydrogen and nitrogen to form ammonia:

3H2(g) + N2(g)→2NH3(g)

How many moles of NH3 can be produced from 24.0 mol of H2 and excess N2?

Express the number of moles to three significant figures.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

                             3H2(g)        +    N2(g)         →              2NH3(g)

Fom the bance equation, 3 mol H2 = 2 mol NH3

Then, 24.o mol H2 = (24.0 x 2 / 3 ) = 16.0 mol of NH3 will be formed.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas , NH3 according to the...
hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas , NH3 according to the equation... 3H2+N2 --->2NH3 1.how many grams of NH3 can be produced from 3.42 mol of N2 and excess H2 2. how many grams of H2 are needed to produce 14.93 g of NH3 ? 3. How many molecules (not moles) of NH3 are produced from 6.04*10^-4 g of H2 ?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g) 1. How many molecules (not moles) of NH3 are produced from 5.25×10−4 g of H2 ?
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g)...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.7 atm N2, 3.2 atm H2, and 0.85 atm NH3 is a) -139.6 b) 0.43 c) -4.63 × 103 d) -44.1 e) -1.08 × 104
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce...
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)⟶2NH3(g) Assume 0.230 mol N2 and 0.758 mol H2 are present initially.PLEASE SHOW steps!! 1)After complete reaction, how many moles of ammonia NH3 are produced? 2)How many moles of H2 remain? 3)How many moles of N2 remain? 4)What is the limiting reactant? nitrogen or hydrogen
part a The reaction of nitrogen and hydrogen to produce ammonia: N2(g) + 3H2(g) ⇌ 2NH3(g)...
part a The reaction of nitrogen and hydrogen to produce ammonia: N2(g) + 3H2(g) ⇌ 2NH3(g) has an equilibrium constant Kc= 1.2 at 375 °C. If the starting concentrations are [H2] = 0.76 M, [N2] = 0.60 M, and [NH3] = 0.48 M, at equilibrium which gases will have increased in concentration and which will have decreased in concentration? a. H2 b. N2 c. NH3 part b When solid sodium bicarbonate is heated the following decomposition reaction occurs: 2NaHCO3(s) ⇌...
N2(g) + 3H2(g) → 2NH3(g) 5.00 g N2 is reacted with 5.00 g H2 How many...
N2(g) + 3H2(g) → 2NH3(g) 5.00 g N2 is reacted with 5.00 g H2 How many mol NH3 can be produced in this reaction?
consider the following reaction: 2NH3 (g) <=> N2 (g) + 3H2 (g) if 7.92 x 10-4...
consider the following reaction: 2NH3 (g) <=> N2 (g) + 3H2 (g) if 7.92 x 10-4 moles of NH3, 0.336 moles of N2 and 0.287 moles of H2 are at equilibrium in a 10.2 L container at 884 K, the value of the equilibrium, Kp, is _
Ammonia, NH3, is produced from the reaction of gaseous nitrogen and hydrogen at high temperatures. 3...
Ammonia, NH3, is produced from the reaction of gaseous nitrogen and hydrogen at high temperatures. 3 H2 (g) + N2 (g)  → 2 NH3 (g) For the reaction of 3.77 g of H2 with 8.66 g of N2, you determined that 21.2 g and 10.5 g of ammonia could be produced, respectively. In the laboratory, you reacted these masses of H2 and N2 and collected 7.70 g of NH3. What is the percentage yield of this reaction to the correct number...
. For the ammonia synthesis reaction, N2+3H2→2NH3, if the rate of reaction with respect to N2...
. For the ammonia synthesis reaction, N2+3H2→2NH3, if the rate of reaction with respect to N2 is -rN2, what is the rate (in terms of -rN2) with respect to a). H2 b.) NH3
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia....
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia. N2 (g) +3 H2 (g) -------------------> 2 NH3 (g) Assume 0.240 mol of N2 and 0.772 mol of H2 are present initially. 1) After complete reaction, how many moles of ammonia are produced? 2) How many moles of H2 remain? 3) How many moles of N2 remain? 4) What is the limiting reactant?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT