What is the mass of 1120cm cube of hydrogen gas at 750mmHg and 40 degree celsius
Use PV = nRT and solve for n = number of mols. Then n = grams/molar mass. You know n and molar mass, solve for gtraams.
To find the mass of a given volume of hydrogen gas at a specific temperature and pressure, you can use the ideal gas law equation: PV = nRT. This equation relates the pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T).
First, let's convert the given values to the required units:
- Convert the volume from cm³ to liters: 1120 cm³ = 1120/1000 = 1.12 liters.
- Convert the pressure from mmHg to atm: 750 mmHg = 750/760 = 0.987 atm.
- Convert the temperature from Celsius to Kelvin: 40°C + 273.15 = 313.15 K.
Now we can use the ideal gas law equation to find the number of moles of hydrogen gas (n). Rearranging the equation, we have:
n = (PV) / (RT)
Substituting the given values:
n = (0.987 atm * 1.12 L) / (0.0821 L·atm/(K·mol) * 313.15 K)
Simplifying the equation:
n = 0.0449 mol
Finally, to calculate the mass of the hydrogen gas, we need to multiply the number of moles (n) by the molar mass of hydrogen (H2), which is approximately 2 g/mol.
Mass = n * molar mass
Mass = 0.0449 mol * 2 g/mol
Mass ≈ 0.0898 g
Therefore, the mass of a 1120 cm³ of hydrogen gas at 750 mmHg and 40 °C is approximately 0.0898 grams.