If 1.50mol of oxygen gas exerts a pressure of 1500mmHg at 20∘C, what is the volume in liters?
PV = nRT
How would I figure out the pressure?
Use google for conversion
1500 mm Hg = 1.97368421 atm = 199 983.553 pascals
To find the volume in liters, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure in atm
V = Volume in liters
n = Number of moles
R = Ideal gas constant (0.0821 L.atm/mol.K)
T = Temperature in Kelvin
First, we need to convert the given pressure from mmHg to atm. Since 1 atm is equal to 760 mmHg, we can use the conversion factor:
1500 mmHg x (1 atm / 760 mmHg) = 1.97 atm
Next, we need to convert the temperature from degrees Celsius to Kelvin. The conversion formula is:
T(K) = T(°C) + 273.15
So, 20 °C + 273.15 = 293.15 K
Now that we have the pressure, temperature, and number of moles (1.50 mol), we can plug them into the ideal gas law equation and solve for the volume:
V = (P * n * R) / T
V = (1.97 atm * 1.50 mol * 0.0821 L.atm/mol.K) / 293.15 K
Calculating this equation will give us the volume in liters.