Answer :
Answer: The pressure exerted by the CO2 gas is 7.03 atmospheres.
Explanation: We can use the ideal gas law to calculate the pressure exerted by the CO2 gas:
PV = nRT
Where:
P is the pressure in atmospheres
V is the volume in liters
n is the number of moles of gas
R is the ideal gas constant (0.08206 L atm/mol K)
T is the temperature in Kelvin
We know the following:
P = ?
V = 50 L
n = (66 g)/(44.01 g/mol) = 1.5 mol
T = -14.5°C + 273.15 K = 258.65 K
Plugging in these values, we get:
P = (1.5 mol)(0.08206 L atm/mol K)(258.65 K) / 50 L
P = 7.03 atm
Therefore, the pressure exerted by the CO2 gas is 7.03 atmospheres.
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Here are the steps on how to calculate the pressure exerted by 66g of CO2 gas at -14.5 degrees C that occupies a volume of 50L:
Calculate the number of moles of CO2 gas.
n = m / M
where:
n is the number of moles of CO2 gas
m is the mass of CO2 gas (66g)
M is the molar mass of CO2 gas (44.01g/mol)
n = 66g / 44.01g/mol = 1.5mol
Calculate the absolute temperature of the CO2 gas.
T = t + 273.15
where:
T is the absolute temperature of the CO2 gas
t is the temperature of the CO2 gas in degrees Celsius (-14.5°C)
T = -14.5°C + 273.15 = 258.65K
Use the ideal gas law to calculate the pressure exerted by the CO2 gas.
PV = nRT
where:
P is the pressure exerted by the CO2 gas
V is the volume of the CO2 gas (50L)
n is the number of moles of CO2 gas (1.5mol)
R is the ideal gas constant (0.08206Latm/molK)
T is the absolute temperature of the CO2 gas (258.65K)
P = nRT / V
P = 1.5mol * 0.08206L*atm/mol*K * 258.65K / 50L
P = 7.43atm
Therefore, the pressure exerted by 66g of CO2 gas at -14.5 degrees C that occupies a volume of 50L is 7.43atm.
Calculate the number of moles of CO2 gas.
n = m / M
where:
n is the number of moles of CO2 gas
m is the mass of CO2 gas (66g)
M is the molar mass of CO2 gas (44.01g/mol)
n = 66g / 44.01g/mol = 1.5mol
Calculate the absolute temperature of the CO2 gas.
T = t + 273.15
where:
T is the absolute temperature of the CO2 gas
t is the temperature of the CO2 gas in degrees Celsius (-14.5°C)
T = -14.5°C + 273.15 = 258.65K
Use the ideal gas law to calculate the pressure exerted by the CO2 gas.
PV = nRT
where:
P is the pressure exerted by the CO2 gas
V is the volume of the CO2 gas (50L)
n is the number of moles of CO2 gas (1.5mol)
R is the ideal gas constant (0.08206Latm/molK)
T is the absolute temperature of the CO2 gas (258.65K)
P = nRT / V
P = 1.5mol * 0.08206L*atm/mol*K * 258.65K / 50L
P = 7.43atm
Therefore, the pressure exerted by 66g of CO2 gas at -14.5 degrees C that occupies a volume of 50L is 7.43atm.
