N2 + 3H2 --> 2NH3 Given the balanced equation above, how many grams of NH3 (theoretical...

Question

Question

N₂ + 3H₂ --> 2NH₃

Given the balanced equation above, how many grams of NH₃ (theoretical yield) can be produced from the reaction of 28.8 g of N₂ and 25 g of H₂?

Answer 1

Answer #1

Please give positive rating. Thanks

Answer:

Add a comment

Answer 2

Similar Homework Help Questions

3H2(g)+N2(g)→2NH3(g) a. How many moles of NH3 can be produced from 13.5 mol of H2 and...

3H2(g)+N2(g)→2NH3(g) a. How many moles of NH3 can be produced from 13.5 mol of H2 and excess N2? b. How many grams of NH3 can be produced from 4.90 mol of N2 and excess H2. c. How many grams of H2 are needed to produce 12.74 g of NH3? d. How many molecules (not moles) of NH3 are produced from 1.05×10−4 g of H2?
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 18.0 mol of H2 and excess N2? Express the number of moles to three significant figures
A. If you have 3.00g of H2, how many grams of NH3 can be produced? B.How...

A. If you have 3.00g of H2, how many grams of NH3 can be produced? B.How many grams of H2 are needed to react with 3.80g of N2? C.How many gramsof NH3 can be produced from 11.6g of H2? Nitrogen gas reacts with hydrogen gas to produce ammonia via the following reaction: N2(g) + 3H2(g)-2NH3(g) Part A If yn

4. From the balanced chemical equation: N2 + 3H2 2 NH3 a) Determine the number moles of NHs produced from the complete reaction of 2.5 moles of H:? [Spts] b) Using the above chemical equation...

4. From the balanced chemical equation: N2 + 3H2 2 NH3 a) Determine the number moles of NHs produced from the complete reaction of 2.5 moles of H:? [Spts] b) Using the above chemical equation determine the number of grams of nitrogen gas (N2) produced when it reacts with 102 g of ammonia (NH3)? [5pts (UPON REQUEST) 4. From the balanced chemical equation: N2 + 3H2 2 NH3 a) Determine the number moles of NHs produced from the complete reaction...
How many moles of NH3 can be produced from 3.25 moles of nitrogen in the following reaction? N2 + 3H2 --> 2NH3

How many moles of NH3 can be produced from 3.25 moles of nitrogen in the following reaction? N2 + 3H2 --> 2NH3
Ammonia can also be synthesized by the reaction: 3H2(g) + N2(g)——2NH3(g) What is the theoretical yield...

Ammonia can also be synthesized by the reaction: 3H2(g) + N2(g)——2NH3(g) What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.42 kg of H2 and 32.5 kg of N2?

Ammonia can also be synthesized by the reaction: 3H2(g)+N2(g)→2NH3(g) What is the theoretical yield of ammonia,...

Ammonia can also be synthesized by the reaction: 3H2(g)+N2(g)→2NH3(g) What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.22 kg of H2 and 33.5 kg of N2?
What is the theoretical yield in grams for this reaction under the given conditions? Express your...

What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units. 3H2(g)+N2(g)→2NH3(g) 1.29 g H2 is allowed to react with 9.92 g N2, producing 2.23 g NH3.
3H2 + N2 -> 2NH3 How many grams of H, are needed to produce 10.31 g...

3H2 + N2 -> 2NH3 How many grams of H, are needed to produce 10.31 g of NH?! Express your answer numerically In grams. View Available Hint(s) IVO AQ RO 0 ? 8H Submit Previous Answers X Incorrect; Try Again; 2 attempts remaining Part D How many molecules (not moles) of NH3 are produced from 3.33x10-4 g of H? Express your answer numerically as the number of molecules. View Available Hint(s) * 0 | ΑΣφ

Consider this reaction: 3H2(g) + N2(g) --> 2NH3(g) First, if 5.00 g of H2 is reacted...

Consider this reaction: 3H2(g) + N2(g) --> 2NH3(g) First, if 5.00 g of H2 is reacted with 21.0 g of N2 determine the identity of the limiting reactant. Second, what theoretical mass of product NH3 would be produced?