Respuesta :
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.
