Question

100 g of nitrogen gas reacts with hydrogen gas to produce 40g of ammonia gas according...

100 g of nitrogen gas reacts with hydrogen gas to produce 40g of ammonia gas according to the equation given below:

N2(g) + 3H2(g) ⇋ 2NH3(g)

Calculate the percentage yield of ammonia

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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(g)+N2(g)→2NH3(g) 1. How many molecules (not moles) of NH3 are produced from 5.25×10−4 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+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 ?
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.60 g H2 is allowed to react with 10.3 g N2, producing 2.24 g NH3. Part A) What...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.71 g H2 is allowed to react with 10.1 g N2, producing 1.36 g NH3. Part A What...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) 1.16 g H2 is allowed to react with 10.2 g N2, producing 2.55 g NH3. The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. Part A: What...
You mix an equal number of moles of nitrogen gas and hydrogen gas in a rigid...
You mix an equal number of moles of nitrogen gas and hydrogen gas in a rigid container such that the total pressure is 2.0 atm. The gases react at a constant temperature to form ammonia and the system reaches equilibrium according to the equation: N2(g) +3H2(g) = 2NH3(g) a. At equilibrium, the total pressure is 1.7335 at a given temperature. Determine the value of Kp for this reaction at this temperature.
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) + 3H2(g) --> 2NH3(g) assume 4 molecules of nitrogen and 9 molecules of hydrogen are present. After complete reaction, how many molecules of ammonia are produced? How many molecules of H2 remain? How many molecules of N2 remain? What is the limiting reactant? hydrogen or nitrogen Please answer all questions and explain this is due today thank you :)
Consider the formation of ammonia from nitrogen gas and hydrogen gas. Balance the equation below. [1]...
Consider the formation of ammonia from nitrogen gas and hydrogen gas. Balance the equation below. [1] N2 +   [3] H2 → [2] NH3 If 5.07g of each reactant are used, what is the mass in grams of ammonia that will be produced?   ___ g What is the percent yield for this reaction if 5.31g of ammonia are actually obtained?   ___ %
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
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation: 3 H2 (g) + N2 (g) → 2 NH3 (g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. What is the maximum theoretical yield in grams if...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT