The pressure exerted by 6.0g of methane gas in a 0.03m3 vessel at 129degreeC is.
PV = nRT
n = grams/molar mass
If you use R as 0.08206 L*atm/mol*K, volume must be changed to L.
1 cubic meter = 1E6 cc and 1000 cc = 1L
To calculate the pressure exerted by the methane gas in the given vessel, we can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure of the gas,
V is the volume of the container,
n is the number of moles of the gas,
R is the ideal gas constant (8.314 J/(mol·K)),
T is the temperature of the gas in Kelvin.
First, let's convert the given temperature to Kelvin:
Temperature in Kelvin = temperature in degree Celsius + 273.15
129°C + 273.15 = 402.15 K
Next, we need to calculate the number of moles of methane gas (CH4) using its molar mass. The molar mass of methane is approximately 16.04 g/mol.
Number of moles = mass of gas / molar mass
Number of moles = 6.0 g / 16.04 g/mol
Now, let's calculate the pressure:
P = (nRT) / V
Substituting the values we have:
P = (number of moles * gas constant * temperature) / volume
P = (number of moles * 8.314 J/(mol·K) * 402.15 K) / 0.03 m³
Now, let's plug in the values and calculate the pressure:
P = (6.0 g / 16.04 g/mol) * 8.314 J/(mol·K) * 402.15 K / 0.03 m³
Solving this equation will give us the pressure exerted by the methane gas in the vessel.