help me please!
What is the pressure in millimeters of mercury of 0.0160 mol of helium gas with a volume of 214 mL at a temperature of 45 ∘C?
Use PV = nRT. You know V(in L), n,R and T(in kelvin). Solve for P in atm and convert to mm. 1 atm = 760 mm Hg.
To find the pressure of the helium gas in millimeters of mercury (mmHg), we can use the ideal gas law equation: PV = nRT, where P represents 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, let's convert the given volume in milliliters to liters.
214 mL = 214/1000 L = 0.214 L
Next, convert the temperature from Celsius to Kelvin.
T(K) = T(°C) + 273.15
T(K) = 45 + 273.15 = 318.15 K
Now we will substitute the given values into the ideal gas law equation.
P * 0.214 L = 0.0160 mol * 0.0821 L atm/(mol K) * 318.15 K
Simplifying the equation:
P * 0.214 L = 0.04091304 L atm
Finally, solve for P by dividing both sides of the equation by 0.214 L.
P = 0.04091304 L atm / 0.214 L
P = 0.191 atm
To convert the pressure to millimeters of mercury (mmHg), we can use the conversion factor: 1 atm = 760 mmHg.
P(mmHg) = 0.191 atm * 760 mmHg / 1 atm
P(mmHg) = 145 mmHg
Therefore, the pressure of 0.0160 mol of helium gas with a volume of 214 mL at a temperature of 45 °C is approximately 145 mmHg.