What would be the density of Hydrogen gas at 500 C and 0.76 atm?
P*molar mass = density*RT
0.024 g/L
To find the density of hydrogen gas at a given temperature and pressure, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
We need to convert the given temperature from Celsius to Kelvin, using the formula:
T (Kelvin) = T (Celsius) + 273.15
So, T = 500 + 273.15 = 773.15 K
Now we can rearrange the ideal gas law equation formula to solve for the number of moles (n) of hydrogen gas:
n = PV / RT
Given:
P = 0.76 atm
V is unknown
R = 0.0821 L·atm/(mol·K)
T = 773.15 K
We will use the density formula that relates the number of moles and volume:
Density (ρ) = molar mass (M) / molar volume (V)
For hydrogen gas, the molar mass (M) is approximately 2 g/mol.
Now, to find the molar volume (V):
V = nRT / P
Substituting the given values:
V = (PV) / (RT)
V = (0.76 atm * V) / (0.0821 L·atm/(mol·K) * 773.15 K)
Simplifying, we can cancel out the units:
V = 0.76 V / 63.66
Now, to find the density (ρ):
ρ = M / V
ρ = 2 g/mol / V
Substituting the value of V into the density equation:
ρ = 2 g/mol / (0.76 V / 63.66)
Finally, we can solve for the density by plugging in the value of V and performing the calculation.