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A 4.35-g piece of solid co2 (dry ice) is allowed to vaporize (change to co2(g)) in a balloon. the final volume of the balloon is 1.00 l at 300. k. what is the pressure of the gas?

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Answer is: the pressure of carbon dioxide is 2.41 atm.
n(CO₂) = m(CO₂) ÷ M(CO₂),

n(CO₂) = 4.35 g ÷ 44 g/mol.

n(CO₂) = 0.098 mol; amount of substance.

V = 1.00, volume of gas.
T = 300 K; temperature.
R = 0.08206 L·atm/mol·K, universal gas constant.
Ideal gas law: p·V = n·R·T.
p = n·R·T / V.
p = 0.098 mol · 0.08206 L·atm/mol·K · 300 K / 1.00 L.
p = 2.41 atm.

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