A 6.08g peice of solid CO2 (dry ice) is allowed to vaporize (change to CO2g) in a balloon. The final volume of the balloon is 1.00 L at 300k. What is the pressure of the gas?
To determine 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.
To calculate the pressure, we need to find the number of moles of CO2 gas released from the solid CO2 (dry ice) and then substitute the other values into the equation.
1. Convert the mass of solid CO2 (dry ice) to moles:
We know the molar mass of CO2 is approximately 44 g/mol.
moles = mass/molar mass = 6.08 g/44 g/mol
2. Calculate the number of moles:
moles = 0.1382 mol (rounded to four decimal places)
3. Determine the pressure:
Plug the values into the ideal gas law equation:
PV = nRT
P * 1.00 L = 0.1382 mol * (0.0821 L * atm/(mol * K)) * 300 K
Note: The ideal gas constant (R) has units of liters * atmospheres / (moles * Kelvin).
4. Solve for pressure (P):
P = (0.1382 mol * 0.0821 L * atm/(mol * K) * 300 K) / 1.00 L
Calculating this equation gives us the pressure of the gas in atmospheres. If you want to convert it to other units, you can use appropriate conversion factors.
It's important to note that the answer depends on the assumption that the CO2 gas behaves ideally under the given conditions.
PV = nRT
Solve for P
V = 1.00 L
n = 6.08/molar mass CO2
R = you know
T = 300K