Question

Suppose 22g of CO₂ at 35°C is in a container of 6L. Assuming ideal gas behavior, calculate the pressure of the gas.

a) State the conditions and assumptions for ideal gas behavior.
b) Outline the relevant formula or equations for calculating gas pressure.
c) Substitute the given values into the formula and solve for the pressure.
d) Explain any additional considerations or steps taken in the calculation.

Answer 1

To calculate the pressure of the gas, use the Ideal Gas Law equation. Convert the temperature to Kelvin and calculate the number of moles using the mass and molar mass. Substitute the values into the equation and solve for pressure.

Step-by-step explanation:

To calculate the pressure of the gas, we can use the Ideal Gas Law equation: PV = nRT. Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Given that the volume is 6L and the temperature is 35°C, we first need to convert the temperature to Kelvin by adding 273.15: 35°C + 273.15 = 308.15K.

Now we need to calculate the number of moles of CO₂. To do this, we can use the formula: moles = mass / molar mass. The molar mass of CO₂ is 44 g/mol, so we have: moles = 22g / 44g/mol = 0.5 mol.

Now we can substitute the values into the Ideal Gas Law equation: P * 6L = 0.5mol * 0.0821 L*atm/(mol*K) * 308.15K. Solving for P: P = (0.5mol * 0.0821 L*atm/(mol*K) * 308.15K) / 6L = 13.45 atm.