Question

Equimolar amounts of Cl₂(g) and CO(g) are injected into an evacuated, rigid container, where they react according to the equation below.

Cl₂(g) + CO(g) => COCl₂(g) ΔHrzn = -109kJ/mol

(a) If 7.0 g of CO(g) is consumed in the reaction with excess Cl₂(g), how many moles of COCl₂(g) are produced?

Answer 1

To find out how many moles of COCl2(g) are produced from 7.0 g of CO(g), we calculate the moles of CO(g) using its molar mass and apply the stoichiometry of the balanced reaction. The result is 0.25 moles of COCl2(g) formed.

Step-by-step explanation:

To determine how many moles of COCl2(g) are produced when 7.0 g of CO(g) is consumed, we first need to know the molar mass of CO(g) and then use the balanced chemical equation provided.

The balanced equation for the reaction is:

Cl2(g) + CO(g) → COCl2(g)

The molar mass of CO(g) is 28.01 g/mol. Based on the stoichiometry of the reaction, one mole of CO(g) reacts with one mole of Cl2(g) to produce one mole of COCl2(g).

Number of moles of CO(g) consumed = mass of CO(g) / molar mass of CO(g)

= 7.0 g / 28.01 g/mol

= 0.25 moles.

Since the reaction is one-to-one, the number of moles of COCl2(g) produced will also be 0.25 moles.