Question

Determine the mass of CO2 produced when 51.2 g of CaO is reacted with 50.0 g of C according to the unbalanced chemical equation:

CaO (s) + C (s) ---> CaC2 (s) + CO2 (g)

Hint: You will need to balance the equation first.

Answer 1

The mass of CO2 produced will be 8.01 grams

Stoichiometric problem

The balanced equation of the reaction is written as:

$2CaO (s) + 5C (s) --- > 2CaC_2 (s) + CO_2 (g)$

The mole ratio of CaO and C is 2:5 from the balanced equation.

Mole of 51.2 g CaO = mass/molar mass = 51.2/56 = 0.91 moles

Mole of 50.0 g C = 50/12 = 4.17 moles

From the mole ratio, 0.91 mole CaO will require 5/2 x 0.91 = 2.28 moles C.

This means 4.17 moles carbon is excessive. In other words, C is the limiting reagent.

The mole ratio of C and CO2 is 5:1. Thus, the equivalent mole of CO2 that will be produced from 0.91 moles C will be:

                                  0.91/5 = 0.182 moles.

Mass of 0.182 moles CO2 = mole x molar mass = 0.182 x 44 = 8.01 grams

More on stoichiometric problems can be found here: https://brainly.com/question/14465605

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