A self-contained underwater breathing apparatus (SCUBA) uses canisters containing potassium superoxide. The superoxide consumes the CO2 exhaled by a person and replaces it with oxygen. 4 KO2(s) + 2 CO2(g) n 2 K2CO3(s) + 3 O2(g) What mass of KO2, in grams, is required to react with 8.90 L of CO2 at 22.0 °C and 767 mm Hg

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Tringa0 Tringa0 · Answer 1 · 2019-07-09T06:43:44+02:00

Answer:

52.0004 grams of mass of potassium superoxide is required

Explanation:

Let moles carbon dioxide gas be n at 22.0 °C and 767 mm Hg occupying 8.90 L of volume.

Pressure of the gas,P = 767 mm Hg = 0.9971 atm

Temperature of the gas,T = 22.0 °C = 295.15 K

Using an ideal gas equation to calculate the number of moles.

[tex]PV=nRT[/tex]

[tex]n=\frac{0.9971 atm\times 8.90 L}{0.0821 atm L/mol K\times 295.15 K}[/tex]

n = 0.3662 mol

[tex]4KO_2(s)+2CO_2(g)\rightarrow 2K_2CO_3(s)+3O_2(g)[/tex]

According to reaction, 2 moles of carbon-dioxide reacts with 4 moles of potassium superoxide.

Then 0.3662 mol of of carbon-dioxide will react with:

[tex]\frac{4}{2}\times 0.3662 mol=0.7324 mol[/tex] of potassium superoxide.

Mass of 0.7324 mol potassium superoxide:

0.7324 mol × 71 g/mol = 52.0004 g

52.0004 grams of mass of potassium superoxide is required.