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Questions and Answers
Match the following quantities with their corresponding values in the context of the ideal gas law solution:
Match the following quantities with their corresponding values in the context of the ideal gas law solution:
Pressure (P) = 1.0 atm Volume (V) = 1.0 L Temperature (T) = 293.15 K Gas constant (R) = 0.082 L atm mol−1 K−1
Match the following terms with their definitions in relation to the calculation of oxygen mass in air:
Match the following terms with their definitions in relation to the calculation of oxygen mass in air:
Mole fraction (x) = Proportion of oxygen in the mixture (0.22) Molecular mass of O2 = 32 g mol−1 Ideal gas behavior = Assumption for calculations Moles of O2 (n) = 0.00924 mol
Match the following calculations to their corresponding results during the exercise:
Match the following calculations to their corresponding results during the exercise:
n = PV/RT = 0.042 mol n(O2) = x(O2) x n = 0.00924 mol Mass O2 = n(O2) x Molecular mass = 0.296 g Temperature conversion = 293.15 K
Match the parameters with their corresponding ideal gas law values:
Match the parameters with their corresponding ideal gas law values:
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Match the following aspects of the tutorial with their respective importance in the solution:
Match the following aspects of the tutorial with their respective importance in the solution:
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Study Notes
Ideal Gas Law
- The ideal gas law equation is PV = nRT
- Where:
- P is pressure in atmospheres (atm)
- V is volume in liters (L)
- n is the number of moles
- R is the ideal gas constant (0.082 L atm mol−1 K−1)
- T is temperature in Kelvin (K)
- To find the number of moles, n, rearrange the equation to n= PV/RT
Converting Temperatures
- To convert from Celsius to Kelvin, add 273.15 to the Celsius temperature
- 20°C is equal to 293.15 K
Calculating Number of Moles
- The number of moles of air can be calculated using the equation n = PV/RT
- Using the values given:
- P = 1.0 atm
- V = 1.0 L
- R = 0.082 L atm mol−1 K−1
- T = 293.15 K
- The number of moles of air is 0.042 mol
Mole Fraction
- The mole fraction of a component in a mixture is the ratio of the number of moles of that component to the total number of moles
- The mole fraction of oxygen (O2) in air is 0.22
- Therefore, the number of moles of oxygen in 1.0 L of air is 0.22 x 0.042 mol = 0.00924 mol
Calculating Mass of Oxygen
- The molecular mass of oxygen (O2) is 32 g mol−1
- The mass of oxygen in 1 L of air is 32 g mol−1 x 0.00924 mol = 0.296 g
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Description
Test your understanding of the Ideal Gas Law with this quiz. It covers the equation PV = nRT, temperature conversions, and the calculation of the number of moles. Challenge your knowledge on mole fractions and air composition as well.
