The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to calculate the number of moles of He gas:
1. Convert the mass of He gas from grams to moles:
4.50 g / 4.00 g/mol = 1.125 mol
Next, we need to convert the temperature from Celsius to Kelvin:
25.0 °C + 273.15 = 298.15 K
Now, we can plug the values into the ideal gas law equation to solve for volume:
V = (nRT) / P
V = (1.125 mol)(0.08206 L.atm/mol.K)(298.15 K) / (770. mmHg * 1 atm / 760 mmHg)
V = (1.125)(0.08206)(298.15) / (770/760)
V = 27.1865 / 1.0001
V = 27.180 L
Therefore, the volume of 4.50 g of He gas at 25.0 °C and 770. mmHg is 27.180 L.
Determine the volume (in L) of 4.50 g of He gas at 25.0 °C and 770. mmHg. Be sure your answer has the correct number of significant figures.
Note: Reference the Fundamental constants and Conversion factors for non-SI units table for additional information.
L
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