Tricia puts 66 g of dry ice (solid CO₂)into a 2.0-L container and seals the top.The dry ice turns to gas at room temperature (20°C).Find the pressure increase in the 2.0-L container.(One mole of CO₂ has a mass of 44 g and R = 0.0821 L·atm/mol·K.Ignore the initial volume of the dry ice. )

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of CO₂ in 66 g: Number of moles = mass/molar mass = 66 g/44 g/mol = 1.5 mol Since all the dry ice will turn into gas, the final number of moles of gas will also be 1.5 mol. Next, we use the ideal gas law to calculate the final pressure: PV = nRT P = nRT/V P = (1.5 mol)(0.0821 L·atm/mol·K)(293 K)/(2.0 L) P = 18.15 atm Finally, we need to subtract the initial atmospheric pressure of 1 atm: P increase = 18.15 atm - 1 atm = 17.15 atm Therefore, the pressure increase in the 2.0-L container is approximately 17 atm, closest to choice C (18 atm).

Tricia Puts 66 G of Dry Ice (Solid CO2)into a 2.0-L

Tricia Puts 66 G of Dry Ice (Solid CO₂)into a 2.0-L