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For the following reaction, give the balanced equation for the reaction.   Consider the following unbalanced equation: NH3(g) → N2(g) + H2(g) How many moles of N2 will be produced by the decomposition of 3.08 moles of ammonia? What information do we need to find how many moles of N2 will be produced?

For the following reaction, give the balanced equation for the reaction.   Consider the following unbalanced equation: NH3(g) → N2(g) + H2(g) How many moles of N2 will be produced by the decomposition of 3.08 moles of ammonia? What information do we need to find how many moles of N2 will be produced?

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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For the following reaction, give the balanced equation for the reaction.

 

Consider the following unbalanced equation:

NH3(g) → N2(g) + H2(g)

How many moles of N2 will be produced by the decomposition of 3.08 moles of ammonia?

What information do we need to find how many moles of N2 will be produced?

a For the following balanced chemical equation, calculate how many moles of products would be produced if 0.310 mol of the first reactant were to react completely. CO2 (9) + 4H2 (g) + CH (g) + 2H,0(1) mol CH, mol H20 Submit b For the following balanced chemical equation, calculate how many moles of products would be produced if 0.329 mol of the first reactant were to react completely. BaCl (ag) + 2AGNO, (ag) + 2AGCI(s) +Ba(NO3)2 (aq) mol AgCl |mol Ba(NO3)2 c For the following balanced chemical equation, calculate how many moles of products would be produced if 0.557 mol of the first reactant were to react completely. C3Hạ (9) + 502 (9) → 4H, O(1) + 3CO2 (9) |mol H20 mol CO2 d For the following balanced chemical equation, calculate how many moles of products would be produced if 0.667 mol of the first reactant were to react completely. 3H, SO, (ag) + 2Fe(s) → Foz (SO4)3 (ag) + 3H2 (9) ]mol Fea (SO4)3 mol H2
Transcribed Image Text:a For the following balanced chemical equation, calculate how many moles of products would be produced if 0.310 mol of the first reactant were to react completely. CO2 (9) + 4H2 (g) + CH (g) + 2H,0(1) mol CH, mol H20 Submit b For the following balanced chemical equation, calculate how many moles of products would be produced if 0.329 mol of the first reactant were to react completely. BaCl (ag) + 2AGNO, (ag) + 2AGCI(s) +Ba(NO3)2 (aq) mol AgCl |mol Ba(NO3)2 c For the following balanced chemical equation, calculate how many moles of products would be produced if 0.557 mol of the first reactant were to react completely. C3Hạ (9) + 502 (9) → 4H, O(1) + 3CO2 (9) |mol H20 mol CO2 d For the following balanced chemical equation, calculate how many moles of products would be produced if 0.667 mol of the first reactant were to react completely. 3H, SO, (ag) + 2Fe(s) → Foz (SO4)3 (ag) + 3H2 (9) ]mol Fea (SO4)3 mol H2
For the following reaction, give the balanced equation for the reaction. Consider the following unbalanced equation: N2(g) + H,(g) – NH;(g) PCla (1) + H2O(1) → H3PO3 (ag) + HC1(9) NH3(g) – N(g) + H,(g) How many moles of H, will be required to react exactly with 3.08 mol N,? What information do we need to find how many moles of H, will be required? molecule(s) PCI, How many moles of N2 will be produced by the decomposition of 3.08 moles of ammonia? molecule(s) H20 What information do we need to find how many moles of N, will be produced? (Select all that apply.) (Select all that apply.) O moles of N, given in the question molecule(s) H3PO3 O moles of NH; given in the question O number of grams present in 1 kilogram |molecule(s) HCl O balanced chemical equation O molar masses of H, and N, O molar masses of NH; and N2 O charges of each element in the reaction O charges of each element in the reaction O balanced chemical equation O number of grams present in 1 kilogram Submit Submit What is the balanced equation for this reaction (in lowest multiple integers)? What is the balanced equation for this reaction (in lowest multiple integers)? N) +C ]NH;) -[ N2(g) +[ |NH3(g) Submit Submit What is the mole ratio between NH; and N, in the balanced equation? What is the mole ratio between N, and H, in the balanced equation? 2 NH3(g) – N(g) + 3 H2(g) N2(3) + 3 H,(g) – 2 NH;(g) mol N2 mol H2 |mol NH3 mol N, Submit Submit How many moles of N, are produced from 3.08 mol NH;? |mol N2 How many moles of H, are required to react exactly with 3.08 mol N,? |mol H, Submit
Transcribed Image Text:For the following reaction, give the balanced equation for the reaction. Consider the following unbalanced equation: N2(g) + H,(g) – NH;(g) PCla (1) + H2O(1) → H3PO3 (ag) + HC1(9) NH3(g) – N(g) + H,(g) How many moles of H, will be required to react exactly with 3.08 mol N,? What information do we need to find how many moles of H, will be required? molecule(s) PCI, How many moles of N2 will be produced by the decomposition of 3.08 moles of ammonia? molecule(s) H20 What information do we need to find how many moles of N, will be produced? (Select all that apply.) (Select all that apply.) O moles of N, given in the question molecule(s) H3PO3 O moles of NH; given in the question O number of grams present in 1 kilogram |molecule(s) HCl O balanced chemical equation O molar masses of H, and N, O molar masses of NH; and N2 O charges of each element in the reaction O charges of each element in the reaction O balanced chemical equation O number of grams present in 1 kilogram Submit Submit What is the balanced equation for this reaction (in lowest multiple integers)? What is the balanced equation for this reaction (in lowest multiple integers)? N) +C ]NH;) -[ N2(g) +[ |NH3(g) Submit Submit What is the mole ratio between NH; and N, in the balanced equation? What is the mole ratio between N, and H, in the balanced equation? 2 NH3(g) – N(g) + 3 H2(g) N2(3) + 3 H,(g) – 2 NH;(g) mol N2 mol H2 |mol NH3 mol N, Submit Submit How many moles of N, are produced from 3.08 mol NH;? |mol N2 How many moles of H, are required to react exactly with 3.08 mol N,? |mol H, Submit
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