for the reaction LiOH + CO2 --> Li2CO3 + H2O?

Question

how many grams of Li2CO3 are produced from the complete reaction of 88.02 g of CO2 ?

Answer 1

Balance the equation
2LiOH + CO2 --> Li2CO3 + H2O

Find the molecular weight of CO2

1 mol C * 12.01g/mol = 12.01g
2 mol O * 16.00g/mol = 32.00g
44.01g/mol CO2

convert from grams CO2 to moles CO2

88.02g CO2 * 1 mol/44.01g = 2 mol CO2

convert from moles CO2 to moles Li2CO3

2 mol CO2 * (1 mol Li2CO3/1 mol CO2) = 2 mol Li2CO3

convert from mol Li2CO3 to grams Li2CO3

first we need the molecular weight

2 mol Li * 6.941g/mol = 13.88g
1 mol C * 12.01g/mol = 12.01g
3 mol O * 16.00g/mol = 48.00g
73.89g/mol Li2CO3

Now we continue

2 mol Li2CO3 * 73.89g/mol LiCO3 = 147.78g Li2CO3 produced

Hope this helps!

Answer 2

Balance the equation to find the mol ratio
2LiOH + CO2 ==> Li2CO3 + H2O
now you have a 1:1 mol ratio
so 88.02 g of CO2 (12.01 + 16 + 16=44.01g) is 2 mol so then find the number of grams in the molar mass of Li2CO3
6.94+6.94+12.01+16+16+16=73.89g
Now since you mol ratio is 1:1 and you have two moles of CO2 you must multiply the Li2CO3 molar mass by 2 as well. 73.89g x 2 = 147.78g
Therefore there are 147.78g of Li2CO3 produced in the reaction