Question

Nitrogen gas occupies a volume of 350 ml at 25 degrees Celsius and one atmospheric pressure. How many moles of nitrogen gas will be there? (Ideal gas constant = 0.082 L atm mol^-1 K^-1).

a) 0.0125 moles

b) 0.025 moles

c) 0.05 moles

d) 0.1 moles

Answer 1

To find the number of moles of nitrogen gas at the given conditions, the ideal gas law is used and the volume is converted from ml to L, and the temperature is converted to Kelvin. After substituting the given values into the ideal gas law, the calculation yields approximately 0.0145 moles, closest to option (a) 0.0125 moles.

Step-by-step explanation:

The question is asking how many moles of nitrogen gas are present in a 350 ml sample at 25 degrees Celsius and one atmospheric pressure using the ideal gas law, which can be represented as 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.

To find the number of moles, you rearrange the ideal gas law to n = PV/RT. In this case, the volume (V) needs to be converted from ml to L, so 350 ml becomes 0.350 L. The temperature (T) must be in Kelvin, so you add 273 to the Celsius temperature, which makes it 298 K (25+273). The ideal gas constant (R) is given as 0.082 L atm mol^-1 K^-1, and the pressure (P) is 1 atm.

Substituting these values into the equation gives n = (1 atm)(0.350 L) / (0.082 L atm mol^-1 K^-1)(298 K). When you perform the calculation, you find that n ≈ 0.0145 moles, which is closest to option (a) 0.0125 moles, assuming slight variations in rounding.