In an experiment, 7.5 mol of a gas are held in a 3.5 L container at 39 c. What pressure does the gas exert if it is assumed to be ideal?
use PV=nRT
make sure that T is in kelvin (K) and you have the correct units for R
To calculate the pressure exerted by 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 in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15:
T = 39°C + 273.15 = 312.15 K.
Now we can plug in the values into the ideal gas law equation:
P * 3.5 L = 7.5 mol * 0.0821 L·atm/mol·K * 312.15 K.
Simplifying the equation:
P * 3.5 L = 7.5 mol * 25.684 L·atm/K.
P * 3.5 L = 192.63 L·atm.
To solve for P, divide both sides of the equation by 3.5 L:
P = 192.63 L·atm / 3.5 L.
Using a calculator, we find that:
P ≈ 55.06 atm.
Therefore, the gas exerts a pressure of approximately 55.06 atm.
To determine the pressure exerted by the gas, we can use the ideal gas law equation, which is:
PV = nRT
Where:
P is the pressure (in units of force per unit area, such as Pa or atm)
V is the volume of the gas (in liters)
n is the number of moles of the gas
R is the ideal gas constant (different values depending on the units used)
T is the temperature of the gas (in Kelvin)
To solve for pressure, we need to rearrange the equation:
P = nRT / V
Now we can substitute the given values into the equation:
n = 7.5 mol
V = 3.5 L
T = 39 °C + 273.15 = 312.15 K (converting from Celsius to Kelvin)
R = 0.0821 L·atm/(mol·K) (ideal gas constant for atm and liter)
Plugging these values into the equation, we get:
P = (7.5 mol) * (0.0821 L·atm/(mol·K)) * (312.15 K) / (3.5 L)
P = 17.727 atm
Therefore, the gas exerts a pressure of approximately 17.727 atm.