Question

Question
1
Question
2
A)
How does stoichiometry support the law of conservation of mass?
(1 point)
It compares the mass of the products to the number of atoms in the products.
It compares the mass of each reactant to the mass of each product.
It compares the mass of the reactants to the number of moles of reactants.
It compares the mass of the products to the mass of the reactants.
A)
Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
N
+ 3H
→ 2NH
Which ratio of components is correct?
(1 point)
2
2
3
For every 3 moles of hydrogen gas, the reaction produces 2 moles of ammonia.
For every 2 moles of nitrogen gas, the reaction requires 3 moles of hydrogen gas.
For every mole of hydrogen gas, the reaction produces 2 moles of ammonia.
For every mole of nitrogen gas, the reaction produces 1 mole of ammonia.
Question
3
Question
4
A)
Nitrogen gas and hydrogen gas react to produce ammonia according to the following equation.
The atomic mass of nitrogen is
. The atomic mass of hydrogen is
. When thereaction produces
grams of ammonia, how many grams of nitrogen were present initially?
(1 point)
N2 + 3H2 → 2NH3
14 g/mol 1 g/mol
68
4
56
12
112
A)
Use this chemical equation to answer the question.
The molar mass of
is
. The molar mass of
is
. Which option shows the correctmolar mass of
?
(1 point)
A + 2B → AB2
A 8 g/mol B 12 g/mol
AB2
32
g
/
mol
20
g
/
mol
40
g
/
mol
64
g
/
mol
Question
5
A)
Hydrogen and oxygen react to produce water according to the following equation.
The molar mass of hydrogen gas (
) is
. The molar mass of oxygen gas (
) is
.When the reaction starts with
grams of oxygen and a sufficient quantity of hydrogen, how manymoles of water are produced?
(1 point)
2H2 + O2 → 2H2O
H2 2 g/mol O2 32 g/mol
64
18
8
2
4

Answer 1

Here are the answers:

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 g

4) 32 g/mol

5) 4 moles