Question

6. A reaction vessel contains 10.0 g of CO and 10.0 g of O2. How many grams of CO2 could be produced according to the following reaction?

2 CO(g) + O2(g) → 2 CO2(g)

Calculate the efficiency of the vessel if 6 g of CO2(g) was collected after the process.

Answer 1

Consider the reaction, 2 CO(g) + O₂(g) ---------> 2 CO₂(g)

molecular weights, 2x(12+16) 32g --------> 2x(12+32)

56g 32g 88g

That is if 56 g of CO can produce 88g CO₂ when reacting with 32 g of oxygen.

So, 1 g of CO require 32/56 g of Oxygen

So 10 g of CO require, 10 x (32/56) = 5.714 g of oxygen.

How much CO₂ will get?

from 56 g CO and 32 g O₂ , 88 g of CO2 will get as the product

So from 10 g CO, you will get (88/56)x10 = 15.7142g of CO₂ will get.

Now, efficiency? instead of 15.714g of CO₂ (expecting), only getting 6g.

Efficiency = =38.1825%.

i hope you got the answer.