Answer :
Final answer:
The volume of H2 gas collected over water at 27°C and 97.5 kPa is 0.0992 L.
Explanation:
First, we need to calculate the number of moles of zinc in 3 g of zinc.
The molar mass of zinc is 65.38 g/mol, so we have:
Number of moles = mass / molar mass
= 3 g / 65.38 g/mol
= 0.04587 mol
Next, we can use the ideal gas law, PV = nRT, to calculate the volume of H2 gas.
The given temperature is 27°C, which we need to convert to Kelvin (27°C + 273.15 = 300.15 K).
The given pressure is 97.5 kPa. The vapor pressure of water at 27°C is 30.6 kPa.
Therefore, the partial pressure of H2 gas is the given pressure minus the vapor pressure of water:
Partial pressure of H2 = 97.5 kPa - 30.6 kPa
= 66.9 kPa
Now we can substitute the values into the ideal gas law equation:
V * 66.9 kPa = 0.04587 mol * 8.314 J/mol·K * 300.15 K
V = (0.04587 mol * 8.314 J/mol·K * 300.15 K) / 66.9 kPa
= 0.0992 L
The volume of H2 gas collected over water at 27°C and 97.5 kPa is 0.0992 L.
