i am not understanding how to solve this how many moles of gas are present in a sample that is at 756 mm Hg pressure, has a volume of 5.3 L, and a temperature of 38 degrees C?
PV=nRT
756mmHG= 0.994atm
38C=311K
(0.994atm)(5.4L)=n(0.08206 L/atm/mol/k)(311K)
n= 0.21 mol
thank you
To solve this problem, you need to use the Ideal Gas Law equation, which is:
PV = nRT
Where:
P is the pressure of the gas (in units of pressure),
V is the volume of the gas (in units of volume),
n is the number of moles of gas,
R is the ideal gas constant (0.0821 L·atm/mol·K or 8.314 J/mol·K),
T is the temperature of the gas (in units of temperature).
In this case, we have:
P = 756 mm Hg
V = 5.3 L
T = 38 °C (which needs to be converted to Kelvin)
First, let's convert the temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature. So, 38 °C + 273.15 = 311.15 K.
Now, we can plug the values into the Ideal Gas Law equation:
(756 mm Hg) * (5.3 L) = n * (0.0821 L·atm/mol·K) * (311.15 K)
Multiply the pressure and volume: 4018.8 mm Hg L = n * 25.530215 L·atm/mol·K
Divide both sides of the equation by the constant (25.530215 L·atm/mol·K):
4018.8 mm Hg L / 25.530215 L·atm/mol·K = n
Simplifying gives:
157.25 mol = n
Therefore, there are approximately 157.25 moles of gas present in the given sample.