what volume would 1.31g of hydrogen occupy at 2.0atm and 127°c?
To determine the volume of a gas, we can use the Ideal Gas Law equation, which is:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, let's convert the given mass of hydrogen (1.31g) into moles. To do this, we need to know the molar mass of hydrogen, which is approximately 2.02 g/mol.
Number of moles = Mass (g) / Molar mass (g/mol)
Number of moles = 1.31g / 2.02 g/mol ≈ 0.649 moles
Now, we have the number of moles of hydrogen (n = 0.649), and we can proceed to calculate the volume.
Since we are given the pressure (P = 2.0 atm) and temperature (T = 127°C), we need to convert the temperature from Celsius to Kelvin.
T (Kelvin) = T (Celcius) + 273.15
T (Kelvin) = 127°C + 273.15 ≈ 400.15 K
Now, we can rearrange the Ideal Gas Law equation to solve for volume:
V = (nRT) / P
Substituting the values we have:
V = (0.649 moles * 0.0821 L·atm / (mol·K) * 400.15 K) / 2.0 atm
After performing the calculation, the volume of 1.31g of hydrogen at 2.0 atm and 127°C is approximately 10.160 L (rounded to three decimal places).