Tricia puts 47 g of dry ice (solid CO₂)into a 4-L container and seals the top.The dry ice turns to gas at room temperature (20°C).Find the pressure increase in the 4-L container.(One mole of CO₂ has a mass of 47 g,R = 0.082 1 L⋅atm/mol⋅K.Ignore the initial volume of the dry ice. ) A) 24 atm B) 6 atm C) 3 atm D) 11 atm E) 19 atm

Question

Quizplus · Accepted Answer

To solve this problem, we can use the ideal gas law: PV = nRT We don't know the final volume or the number of moles of gas, but we do know the initial number of moles of dry ice. We can use the fact that dry ice (CO₂) sublimes into one mole of gas: CO₂(s) → CO₂(g) So, we have one mole of gas in a 4 L container at 20°C. We can plug in the values we know: P(4 L) = (1 mol)(0.0821 L⋅atm/mol⋅K)(293 K) Solving for P, we get: P = 6 atm Therefore, the pressure increase in the 4-L container is 6 atm. The answer is B.

Tricia Puts 47 G of Dry Ice (Solid CO2)into a 4-L

Tricia Puts 47 G of Dry Ice (Solid CO₂)into a 4-L