Calculate the pressure exerted by 1.2 mol\rm mol of gas in a volume of 28.2 L\rm L and at a temperature of 334 K\rm K.
Use PV = nRT; solve for P
To calculate the pressure exerted by a gas, you need to use the ideal gas law equation:
PV = nRT
Where:
P is the pressure (in units of pressure, such as Pascal or atm)
V is the volume (in units of liters or cubic meters)
n is the number of moles of gas
R is the ideal gas constant (which depends on the units being used)
T is the temperature (in units of Kelvin)
Given the following values:
n = 1.2 mol
V = 28.2 L
T = 334 K
We can plug the values into the equation and solve for P:
P * 28.2 L = 1.2 mol * R * 334 K
To find the pressure, you need to know the value of the ideal gas constant, which depends on the units being used for pressure and volume. In this case, let's use the ideal gas constant with units of atm·L/(mol·K).
Plugging in the values and solving for P:
P * 28.2 L = 1.2 mol * (0.0821 atm·L/(mol·K)) * 334 K
P * 28.2 L = 32.8612 atm·L
P = 32.8612 atm·L / 28.2 L
P ≈ 1.165 atm
Therefore, the pressure exerted by 1.2 mol of gas in a volume of 28.2 L and at a temperature of 334 K is approximately 1.165 atm.