At 0.00 °C and 1.00 atm pressure, a sample of gas occupies 20.0 mL. If the temperature is increased to 30.0°C and the entire gas sample is transferred to a 30.0-mL container. The pressure of the gas in the new container is:
To find the pressure of the gas in the new container, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
First, we need to determine the number of moles of gas in the initial container at 0.00 °C:
P1V1 = nRT1
1.00 atm * 20.0 mL = n * 0.0821 L.atm/mol.K * 273 K
n = (1.00 atm * 20.0 mL) / (0.0821 L.atm/mol.K * 273 K)
n = 0.74 mol
Next, we need to use the ideal gas law to find the pressure of the gas in the new container at 30.0 °C:
P2V2 = nRT2
P2 * 30.0 mL = 0.74 mol * 0.0821 L.atm/mol.K * 303 K
P2 = (0.74 mol * 0.0821 L.atm/mol.K * 303 K) / 30.0 mL
P2 = 1.54 atm
Therefore, the pressure of the gas in the new container at 30.0°C is 1.54 atm.