How many moles of helium gas occupy 22.4 l at 0oC at 1 atm. Pressure
Correct answer: C. 1.0
- A. 011
- B. 0.90
- C. 1.0
- D. 1.11
Explanation
We can use the ideal gas law to solve this problem. The ideal gas law relates the pressure (P), volume (V), temperature (T), and number of moles (n) of an ideal gas:PV = nRTwhere:R is the ideal gas constant (approximately 0.08206 L atm/mol K)T is the temperature in Kelvin (0°C = 273.15 K)We are given:V = 22.4 LP = 1 atmT = 273.15 KWe need to find n (number of moles). Rearranging the ideal gas law and plugging in the values:n = PV / RTn = (1 atm)(22.4 L) / (0.08206 L atm/mol K)(273.15 K)n ≈ 1.00 molTherefore, 1.0 moles of helium gas occupy 22.4 L at 0°C and 1 atm pressure
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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