Question

Assuming all volume measurements are made at the same temperature and pressure, how many liters of oxygen gas would it take to react completely with 7.25 liters of hydrogen gas? Show all of the work used to solve this problem.. . Unbalanced equation: H2 (g) + O2 (g) -> H2 O(g)

Answer 1

Answer: 3.625 L of oxygen gas will be required.

Step-by-step explanation:

We know that:

1 mole of a gas occupies 22.4 Liters of gas.

For the reaction of formation of water, the balanced equation follows:

`2H_2+O_2\rightarrow 2H_2O`

By Stoichiometry of the reaction:

2 moles of hydrogen gas reacts with 1 mole of oxygen gas.

This means that 44.8 L of hydrogen gas reacts with 22.4 L of oxygen gas.

So, 7.25 L of hydrogen gas will react with = [tex]\frac{22.4L}{44.8L}\times 7.25L=3.625L[tex] of oxygen gas.

Hence, 3.625 L of oxygen gas will be required.

Answer 2

1. Balanced equation 2 H2 + O2 --> 2 H2O

7.25 L H2 ( 1 L O2 / 2 L H2) = 3.62 L O2

2. M1V1 = M2V2
12.3 M X V1 = 1.2 M X 12.4 L

V1 = 1.21 L

3. The solution containing calcium chloride will have a higher boiling point because it produces more particles when it dissolves.