What is the pressure in millimeters of mercury of 0.0140mol of helium gas with a volume of 222mL at a temperature of 30∘C?
PV=nRT
Just plug in your numbers and solve for P.
To find the pressure in millimeters of mercury (mmHg) of the given amount of gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in this case, in mmHg)
V = Volume (in this case, in liters)
n = Number of moles of gas
R = Ideal gas constant (0.0821 L·atm/(mol·K) or 62.36 L·mmHg/(mol·K))
T = Temperature (in Kelvin)
First, let's convert the given values to the appropriate units.
Volume: 222 mL = 0.222 L
Temperature: 30∘C = 30 + 273.15 = 303.15 K
Now, substituting the values into the ideal gas law equation, we have:
P * 0.222 = 0.0140 * 0.0821 * 303.15
Solving for P:
P = (0.0140 * 0.0821 * 303.15) / 0.222
Now, let's calculate the pressure:
P = 3.07008
Therefore, the pressure of 0.0140 mol of helium gas with a volume of 222 mL at a temperature of 30∘C is approximately 3.07 mmHg.