Multiple Choice
Benzene has a heat of vaporization of 30.72 kJ/mol and a normal boiling point of 80.1 °C. At what temperature does benzene boil when the external pressure is 410 torr?
7. Gases
The Ideal Gas Law
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Using the Ideal Gas Law, how many moles of N2 (g) are present in 1.00 L of N2 (g) at 100.°C and 1.00 atm?
A
0.200 moles
B
0.0821 moles
C
0.100 moles
D
0.0406 moles
Verified step by step guidance1
Start by recalling the Ideal Gas Law equation: \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is temperature in Kelvin.
Convert the given temperature from Celsius to Kelvin using the formula: \( T(K) = T(°C) + 273.15 \). For 100.°C, calculate \( T(K) \).
Identify the values given in the problem: \( P = 1.00 \text{ atm} \), \( V = 1.00 \text{ L} \), and \( T \) in Kelvin from the previous step. The ideal gas constant \( R \) is \( 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \).
Rearrange the Ideal Gas Law to solve for \( n \), the number of moles: \( n = \frac{PV}{RT} \).
Substitute the known values into the rearranged equation and solve for \( n \) to find the number of moles of \( N_2 \).
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