Question

Part B. Solid lithium hydroxide is used to "scrub" CO2 from the air in spacecraft and submarines; it reacts with the CO2 to produce lithium carbonate and water. What volume in liters of CO2 at 21°C and 736 torr can be removed by reaction with 439 g of lithium hydroxide? Enter to 3 sig figs.

Part C. The alkali metals react with the halogens to form ionic metal halides. What mass in g of sodium chloride forms when 5.98 L of chlorine gas at 0.841 atm and 26.8°C reacts with 11.8 g of sodium. Write a balanced chemical equation. Enter to 1 decimal place.

Answer 1

B)

The balanced equation is

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

2 moles of LiOH react with 1 moles of CO2.

439/23.95 moles of LiOH reacts with = 439 x1 / 23.95 x 2

= 9.16moles of CO2

The volume of CO2 is calculated by using the ideal gas equation

PV = nRT

Volume V = 9.16 mol x 0.0821 L.ATm/mol.K x 294 K / ( 733/760) atm

= 229.366 L

C)

The balanced chemical equation is

2Na (s) + Cl2(g) -------------> 2 NaCl (s)

moles of chlroine taken = PV/RT

= 0.841 atm x 5.98 L / 0.0821L.atm/mol.K x 299.8 K

= 0.204 mol

moles sodium taken = 11.8/23 =0.51

2Na (s) + Cl2(g) -------------> 2 NaCl (s)

0.51 moles 0.204 0 initial

0.102 0 2x0.204 after reaction

Thus mass of NaCl formed = moles x molar mass

= 2x0.204 mol x 58.5g/mol

= 23.868 g