객관식
Given that 0.10 mol of nitrogen gas undergoes two processes, which of the following statements about the final pressure of the gas is correct if the volume doubles and the temperature remains constant?
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7. Gases
The Ideal Gas Law
객관식
How many liters of HNO3 gas, measured at 28.0 ºC and 780 torr, are required to prepare 2.30 L of 4.15 M solution of nitric acid?
A
56 L
B
62 L
C
189 L
D
230 L
E
262 L
검증된 단계별 안내1
First, calculate the number of moles of HNO3 needed using the molarity formula: \( M = \frac{n}{V} \), where \( M \) is the molarity, \( n \) is the number of moles, and \( V \) is the volume in liters. Rearrange to find \( n = M \times V \). Substitute \( M = 4.15 \text{ M} \) and \( V = 2.30 \text{ L} \) to find \( n \).
Next, use the ideal gas law to find the volume of HNO3 gas required. The ideal gas law 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.
Convert the given temperature from Celsius to Kelvin by using the formula \( T(K) = T(°C) + 273.15 \). For this problem, \( T = 28.0 + 273.15 \).
Convert the pressure from torr to atm, since the ideal gas constant \( R \) is typically given in terms of atm. Use the conversion factor \( 1 \text{ atm} = 760 \text{ torr} \). Therefore, \( P = \frac{780}{760} \text{ atm} \).
Rearrange the ideal gas law to solve for \( V \): \( V = \frac{nRT}{P} \). Substitute the values for \( n \), \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \), \( T \), and \( P \) to find the volume of HNO3 gas required.
