Question

The main engines of the U.S. space shuttle are powered by liquid hydrogen and liquid
oxygen. If 1.02 x 105 kg of liquid hydrogen is carried on a particular launch, what mass of
liquid oxygen is necessary for all the hydrogen to burn. The equation for the reaction is,
2H
+ O2 → 2H2O
(g
(g)
(Ans: 8.16 * 105 kg oxygen)

Answer 1

Answer:

8.16 * 10^5 kg oxygen or 8.16 * 10^8 g oxygen

Explanation:

Acc. to equation of reaction; 4 g of H2 are burnt in presence of 32 g of O2. Given data states that if 1.02 x 10^8 grams of H2 are taken then x grams of O2 is required....

• (32/4) × 1.02 x 10^8 ⇒ 8.16 * 10^8 g oxygen or 8.16 * 105 kg oxygen

Answer 2

Given:

Mass of liquid hydrogen = 1.02 X 10⁵ Kg

To Find:

The mass of liquid oxygen required to completely react with the hydrogen

Solution:

The balanced reaction of hydrogen with oxygen is as follows:

2 H₂ + O₂  -> 2 H₂O

From the above reaction, we can conclude that two moles of hydrogen react completely with 1 mole of oxygen to form two moles of water.

We know that the molar mass of Hydrogen is 2g and that of oxygen is 32g.

So, 2 X 2 g of Hydrogen reacts with 32g of Oxygen

So using the unitary method,

the mass of oxygen needed to react with 1.02 X 10⁵ Kg=

32 X 1.02 X 10⁵ Kg / 4

= 8 X 1.02 X 10⁵ Kg

= 8.16 X 10⁵ Kg

Hence, 8.16 X 10⁵ Kg of liquid oxygen is required.