A 35.1 g sample of solid CO2 (dry ice) is added to a container at a temperature of 100 K with a volume of 4.0 L. If the container is evacuated (all of the gas is removed), sealed, and then allowed to warm to room temperature (𝑇=298 K) so that all of the solid CO2 is converted to a gas, what is the pressure inside the container?

Verified step by step guidance

Step 1: First, we need to calculate the number of moles of CO2. We can do this by using the molar mass of CO2, which is 44.01 g/mol. The formula to calculate the number of moles is: n = mass / molar mass.

Step 2: Next, we need to convert the volume of the container from liters to cubic meters, as the ideal gas law requires the volume to be in cubic meters. We can do this by using the conversion factor 1 L = 0.001 m^3.

Step 3: Now, we can use the ideal gas law to calculate the pressure. The ideal gas law is: P = nRT / V, where P is the pressure, n is the number of moles, R is the ideal gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, and V is the volume in cubic meters.

Step 4: Substitute the values of n, R, T, and V into the ideal gas law equation to calculate the pressure.

Step 5: The pressure will be in Pascals (Pa). If you need the pressure in another unit, such as atmospheres or torr, you will need to convert it using the appropriate conversion factor.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law is essential for calculating the pressure of gases under various conditions, particularly when transitioning from solid to gas states.

Phase Change

Phase change refers to the transformation of a substance from one state of matter to another, such as from solid to gas. In this scenario, dry ice (solid CO2) sublimates directly into gas when heated. Understanding phase changes is crucial for predicting how substances behave under different temperature and pressure conditions, especially in thermodynamic processes.

Molar Mass and Moles Calculation

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. For CO2, the molar mass is approximately 44.01 g/mol. To find the number of moles in a given mass, the formula n = mass/molar mass is used. This calculation is vital for determining the amount of gas produced from the sublimation of dry ice, which is necessary for applying the Ideal Gas Law.

Recommended video:

Guided course

03:12

Molar Mass Calculation Example

Related Practice

Textbook Question

A scuba diver’s tank contains 0.29 kg of O2 compressed into a volume of 2.3 L. b. What volume would this oxygen occupy at 26°C and 0.95 atm?

Textbook Question

An aerosol spray can with a volume of 250 mL contains 2.30 g of propane gas (C3H8) as a propellant. a. If the can is at 23°C, what is the pressure in the can?

Textbook Question

An aerosol spray can with a volume of 250 mL contains 2.30 g of propane gas (C3H8) as a propellant. c. The can’s label says that exposure to temperatures above 130°F may cause the can to burst. What is the pressure in the can at this temperature?

Textbook Question

A 334-mL cylinder for use in chemistry lectures contains 5.225 g of helium at 23°C. How many grams of helium must be released to reduce the pressure to 75 atm assuming ideal-gas behavior?

Textbook Question

Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 24°C. b. What volume will the Cl2 occupy at STP?

Textbook Question