Multiple Choice
When 0.670 g argon is added to a 500 cm3 container with a sample of oxygen gas, the total pressure of the gases is found to be 1.52 atm at a temperature of 340 K. What is the mass of the oxygen gas in the bulb?
11 Gases
The Ideal Gas Law
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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
Verified step by step guidance1
Start by understanding that you need to find the volume of HNO3 gas required to prepare a solution. The solution's concentration is given as 4.15 M, which means 4.15 moles of HNO3 per liter of solution.
Calculate the total moles of HNO3 needed using the formula: \( \text{moles} = \text{molarity} \times \text{volume} \). Here, the volume of the solution is 2.30 L.
Use the Ideal Gas Law to find the volume of HNO3 gas. The Ideal Gas Law is \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is moles, \( R \) is the gas constant, and \( T \) is temperature in Kelvin.
Convert the given temperature from Celsius to Kelvin using the formula: \( T(K) = T(°C) + 273.15 \). Also, convert the pressure from torr to atm using the conversion: \( 1 \text{ atm} = 760 \text{ torr} \).
Rearrange the Ideal Gas Law to solve for volume \( V \): \( V = \frac{nRT}{P} \). Substitute the values for \( n \), \( R \) (0.0821 L·atm/mol·K), \( T \), and \( P \) to find the volume of HNO3 gas required.
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