Hello! I am struggling a bit with this problem
A gas sample occupies 51.6 L at a pressure of 0.841 atm and 39.6 ºC. What is the amount of gas (mol) in this sample?
PV = nRT
What's the trouble. Plug in P, V, R, T and solve for n. Remember to convert C to Kelvin
Hello! I can help you with that problem. To find the amount of gas (mol) in a sample, we can use the Ideal Gas Law equation, which is:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in L)
n = amount of gas in moles
R = ideal gas constant (0.0821 L*atm/(mol*K))
T = temperature of the gas (in Kelvin)
In this case, we are given the pressure (P), volume (V), and temperature (T) of the gas sample. Thus, we can rearrange the Ideal Gas Law equation to solve for the amount of gas (n):
n = PV / RT
Now, let's gather the known values from the problem:
P = 0.841 atm
V = 51.6 L
T = 39.6 ºC
To use the Ideal Gas Law equation, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(ºC) + 273.15
So, by substituting the values into the equation, we get:
n = (0.841 atm * 51.6 L) / (0.0821 L*atm/(mol*K) * (39.6 + 273.15) K)
Now, you can calculate the value of n.