The volume occupied by 2.8 g of N2 at STP
Correct answer: A. 2.24dm3
- A. 2.24dm3
- B. 22.4 dm³
- C. 1.12 dm³
- D. 11.2 cm³
Explanation
To find the volume occupied by a gas at Standard Temperature and Pressure (STP), we can use the ideal gas law and the molar volume of a gas at STP.STP conditions are defined as a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (atm). The molar volume of any gas at STP is approximately 22.4 liters per mole.Given the mass of nitrogen gas (N2) as 2.8 g, we first need to determine the number of moles of N2:Number of moles = Mass/ Molar massThe molar mass of nitrogen gas (N2) is approximately 28 g/mol.Number of moles = 2.8 g / 28 (g/mol) = 0.1 molNow, we can use the molar volume of a gas at STP to find the volume:Volume =Number of moles* Molar volume at STPVolume = 0.1 * 22.4 dm^3 / molVolume = 0.1 * 2.24 dm^3Therefore, the correct answer is (a) 2.24 dm³.
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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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