forgot to add
Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
N2 + 3H2 → 2NH3
The atomic mass of nitrogen is 14 g/mol. The atomic mass of hydrogen is 1 g/mol. When the reaction produces 68 grams of ammonia, how many grams of nitrogen were present initially?
4
112
56
12
11 answers
molar mass of NH3 = 14+3 = 17 grams/mol
68 grams / 17 grams/mol = 4 mols of NH3
that needs 2 mols of N2
2 * 2 * 14 = 56 grams of N2
68 grams / 17 grams/mol = 4 mols of NH3
that needs 2 mols of N2
2 * 2 * 14 = 56 grams of N2
Eeeeeeeeeeeeee
1. It compares the mass of the products to the mass of the reactants.
2. For every 3 moles of hydrogen gas, the reaction produces 2 moles of ammonia.
3. 56
4. 32 g/mol
5. 4
2. For every 3 moles of hydrogen gas, the reaction produces 2 moles of ammonia.
3. 56
4. 32 g/mol
5. 4
i did it is correct 5/5 thanks for the help.
i did it is right 100% honest
For those who want to see the questions with answers.
1. How does stoichiometry support the law of conservation of mass?
Ans: (A) It compares the mass of the products to the mass of the reactants.
2. Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
N2 + 3H2 → 2NH3
Which ratio of components is correct?
Ans: (B) For every 3 moles of hydrogen gas, the reaction produces 2 moles of ammonia.
3. Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
N2 + 3H2 → 2NH3
The atomic mass of nitrogen is 14 g/mol. The atomic mass of hydrogen is 1 g/mol. When the reaction produces 68 grams of ammonia, how many grams of nitrogen were present initially?
Ans: (C) 56
4.Elements A and B react according to the balanced equation shown.
2A + 3B2 → 2AB2
The molar mass of A is 8 g/mol. The molar mass of B is 12 g/mol. Which option shows the correct molar mass of AB2?
Ans: (B) 32g/mol
5.Hydrogen and oxygen react to produce water according to the following equation.
2H2 + O2 → 2H2O
The molar mass of hydrogen gas (H2) is 2 g/mol. The molar mass of oxygen gas (O2) is 32 g/mol. When the reaction starts with 64 grams of oxygen and a sufficient quantity of hydrogen, how many moles of water are produced?
5. (C) 4
1. How does stoichiometry support the law of conservation of mass?
Ans: (A) It compares the mass of the products to the mass of the reactants.
2. Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
N2 + 3H2 → 2NH3
Which ratio of components is correct?
Ans: (B) For every 3 moles of hydrogen gas, the reaction produces 2 moles of ammonia.
3. Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
N2 + 3H2 → 2NH3
The atomic mass of nitrogen is 14 g/mol. The atomic mass of hydrogen is 1 g/mol. When the reaction produces 68 grams of ammonia, how many grams of nitrogen were present initially?
Ans: (C) 56
4.Elements A and B react according to the balanced equation shown.
2A + 3B2 → 2AB2
The molar mass of A is 8 g/mol. The molar mass of B is 12 g/mol. Which option shows the correct molar mass of AB2?
Ans: (B) 32g/mol
5.Hydrogen and oxygen react to produce water according to the following equation.
2H2 + O2 → 2H2O
The molar mass of hydrogen gas (H2) is 2 g/mol. The molar mass of oxygen gas (O2) is 32 g/mol. When the reaction starts with 64 grams of oxygen and a sufficient quantity of hydrogen, how many moles of water are produced?
5. (C) 4
ilysm i swear
Help is 100% correct
I didn’t look at the answer at all - :))
You guys are all so incredible. i hope you do well in life, you really deserve it ^^
3 answers