Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22°C and 100 kPa?
no choices. You should check after posting to make sure the question is stated properly.
Use PV=nRT
P is pressure in atm
V is what you are looking for
n is number of moles (1.5 mol)
R is a constant( .08206)
And T is temperature in Kelvin (22+273)
PLUG AND CHUG
To determine the volume of a gas sample, we can use the ideal gas law equation:
PV = nRT
where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the ideal gas constant
T is the temperature of the gas in Kelvin
To set up the equation correctly, we need to rearrange the equation to solve for V (volume):
V = (nRT) / P
Given:
n = 1.5 moles (number of moles of oxygen gas)
T = 22°C (temperature in Celsius)
P = 100 kPa (pressure in kilopascals)
However, we need to convert the temperature from Celsius to Kelvin by adding 273.15:
T = 22°C + 273.15 = 295.15 K
Now we have all the necessary values, so let's substitute them into the equation:
V = (1.5 moles * 0.0821 L⋅atm/(mol⋅K) * 295.15 K) / 100 kPa
Here, we have used the value of the ideal gas constant, which is approximately 0.0821 L⋅atm/(mol⋅K).
Now, let's simplify the equation:
V = 1.219615 L
Therefore, the equation set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22°C and 100 kPa is:
V = (1.5 * 0.0821 * 295.15) / 100