Question

Carbon dioxide reacts with lithium hydroxide to produce lithium carbonate and water.

What mass of lithium hydroxide would be required to react with 1.00 x 103 grams of carbon dioxide?

Answer 1

To find the mass of lithium hydroxide required to react with 1.00 x 10^3 grams of carbon dioxide, we can use the balanced chemical equation and stoichiometry calculations. The mass of lithium hydroxide required is 47.90 grams.

Step-by-step explanation:

To find the mass of lithium hydroxide required to react with 1.00 x 10^3 grams of carbon dioxide, we need to first determine the balanced chemical equation for the reaction:

CO2 + 2LiOH → Li2CO3 + H2O

From the equation, we can see that 2 moles of LiOH react with 1 mole of CO2. To find the number of moles of CO2 in 1.00 x 10^3 grams, we divide the mass of CO2 by its molar mass:

Molar mass of CO2 = 12.01 g/mol (C) + 2(16.00 g/mol) = 44.01 g/mol

Moles of CO2 = 1.00 x 10^3 g / 44.01 g/mol = 22.72 mol

Since the stoichiometric ratio is 1:2 for CO2 and LiOH, we can calculate the mass of LiOH required:

Mass of LiOH = 2 moles of LiOH x molar mass of LiOH = 2(23.95 g/mol) = 47.90 g

Answer 2

1.08827 x 10^3 g.

Step-by-step explanation:

The equation for the reaction is:

2LiOH + CO2 ----> Li2CO3 + H2O

Using the molar masses:

CO2 = 12.011 + 2* 16 = 44.011.

LiOH = 6.94 + 1.008 + 16 = 23.948

S0 44.011 of CO2 reacts with 2*23.948 g of LiOH

1.00 *10^3 g CO2 reacts with 2*23.948 * 1.00 *10^3 / 44.011

= 1088.27 g LiOH.