How many moles of CO2 can be produced by the complete reaction of 1.0 g of lithium carbonate with excess hydrochloric acid (balanced chemical reaction is given below) ? Li2CO3 (s) + 2HCl (aq) - -> 2LiCl (aq) + H2O (l) + CO2 (g) Question 1 options: 1.7 g 1.1 g 0.60 040 g

Question

Chemistry

Phoenix Lynn

2 August, 17:21

How many moles of CO2 can be produced by the complete reaction of 1.0 g of lithium carbonate with excess hydrochloric acid (balanced chemical reaction is given below) ? Li2CO3 (s) + 2HCl (aq) - -> 2LiCl (aq) + H2O (l) + CO2 (g) Question 1 options: 1.7 g 1.1 g 0.60 040 g

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Answers (1)

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Sandra Johnson · Answer 1

Answer:Mass of CO2 = 0.60g

Explanation:

Given the chemical rection

Li2CO3 (s) + 2HCl (aq) - -> 2LiCl (aq) + H2O (l) + CO2 (g

No of moles = mass / molar mass

molar mass Li2CO3 = Molecular mass calculation: 6.941 x 2 + 12.0107 + 15.9994 x 3 =

= 73.8909 g/mol

therefore Number of moles Li2CO3 = 1.0g / 73.89 g/mol

= 0.0135 moles Li2CO3

From our given Balanced equation, shows that

Li2CO3 (s) + 2HCl (aq) - -> 2LiCl (aq) + H2O (l) + CO2 (g

1 mole Li2CO3 produces 1 mole CO2

therefore 0.0135 mol Li2CO3 will produce 0.0135 moles of CO2

Also

No of moles = mass / molar mass

Mass = No of moles x molar mass

molar mass of CO2=12.0107 + 15.9994 x 2=44.0095 g/mol

Mass of CO2 = 0.0135 X 44.0095 g/mol = 0.594≈0.60g