nitrogen gas is at 2.00. c, 2.00 atm pressure and occupies a volume of 10.01. Assume nitrogen is an ideal gas, how many moles of the gas are present?
What does 200.c, mean?
10.01 what?
To determine the number of moles of an ideal gas, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin
In this case, we have:
P = 2.00 atm
V = 10.01 L
T = 2.00 °C
First, let's convert the temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 2.00 + 273.15
T(K) = 275.15 K
Now, we can rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / RT
Substituting the provided values:
n = (2.00 atm) * (10.01 L) / (0.0821 L·atm/(mol·K)) * (275.15 K)
By multiplying the values and dividing appropriately:
n ≈ 0.074 moles
Therefore, approximately 0.074 moles of nitrogen gas are present.