Use the ideal gas equation to answer this question. (Recall that R is .0821 L · atm/K · mol. ) What pressure is exerted by .35 moles of a gas at 23 0 C if it is held in a container with a volume of 2.3 liters?
What's your problem with this? Substitute te numbers and calculate it. The 23.0C must be converted to kelvin.
To answer this question using the ideal gas equation, we need to use the formula:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
Given the following values:
n = 0.35 moles
V = 2.3 liters
R = 0.0821 L · atm/K · mol
T = 23°C (temperature in Celsius)
First, we need to convert the temperature to Kelvin because the ideal gas equation requires temperature in Kelvin. To convert from Celsius to Kelvin, we add 273.15:
T = 23°C + 273.15 = 296.15 K
Now we can substitute the values into the ideal gas equation:
PV = nRT
P * 2.3 = 0.35 * 0.0821 * 296.15
P * 2.3 = 8.94287
Divide both sides by 2.3 to solve for P:
P = 8.94287 / 2.3
P ≈ 3.88 atm
Therefore, the pressure exerted by 0.35 moles of gas at 23°C in a container with a volume of 2.3 liters is approximately 3.88 atm.