Question

Consider the reaction: 2CO(g) + O2(g) → 2CO2(g). Given an initial mass of 10.91 g CO, an excess of O2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of CO2 produced by the reaction.

Answer 1

To calculate the mass of CO2 produced from 10.91 g of CO with excess O2, the molar mass of CO is used to find the number of moles, which is then converted to the mass of CO2 using CO2's molar mass, according to the stoichiometry of the reaction.

Step-by-step explanation:

Calculating the mass of CO2 produced in a chemical reaction requires the application of the law of conservation of mass, which implies that the mass of the reactants is equal to the mass of the products.

Given the reaction 2CO(g) + O2(g) → 2CO2(g), and an initial mass of 10.91 g of CO, with excess O2, the calculation steps are as follows:

1. First, find the molar mass of CO which is 28.01 g/mol.
2. Divide the initial mass of CO by its molar mass to get the number of moles of CO, which is 10.91 g / 28.01 g/mol.
3. Use the stoichiometry of the reaction to relate moles of CO to moles of CO2, which follows a 1:1 ratio based on the balanced equation.
4. Finally, multiply the moles of CO2 by its molar mass, which is 44.01 g/mol, to find the mass of CO2 produced.