Multiple Choice
What temperature (in °C) did an ideal gas shift to if it was initially at -18.0 °C at 4.62 atm and 35.0 L, and the pressure was changed to 8.31 atm and the volume changed to 25.0 L?
7. Gases
The Ideal Gas Law
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Using the Ideal Gas Law, what is the volume of 6.79 g of N₂ gas at 110°C and 760 torr?
A
5.60 L
B
3.90 L
C
4.50 L
D
6.80 L
Verified step by step guidance1
Convert the mass of N₂ gas to moles using the molar mass of N₂. The molar mass of N₂ is approximately 28.02 g/mol. Use the formula: \( \text{moles of N}_2 = \frac{\text{mass of N}_2}{\text{molar mass of N}_2} \).
Convert the temperature from Celsius to Kelvin, as the Ideal Gas Law requires temperature in Kelvin. Use the formula: \( T(K) = T(°C) + 273.15 \).
Convert the pressure from torr to atmospheres, since the Ideal Gas Law uses pressure in atmospheres. Use the conversion: \( 1 \text{ atm} = 760 \text{ torr} \).
Use the Ideal Gas Law equation \( PV = nRT \) to solve for the volume \( V \). Rearrange the equation to \( V = \frac{nRT}{P} \), where \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.
Substitute the values for \( n \), \( R \), \( T \), and \( P \) into the rearranged Ideal Gas Law equation to calculate the volume \( V \) of the gas.
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