CHEM103: Gas Stoichiometry/Dalton's Law 13.3-13.4 Practice with the Correct Answer

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A typical equation stoichiometry problem is solved by starting with a measurable quantity of one compound, converting it to moles. Then, from the balanced equation, we calculate moles of the second co... mpound. Finally, we convert moles back to another measurable property. For solids and liquids, the common measurable quantity is ______. -CORRECT ANSWER-mass When working with gases, it is often necessary to use ______ as a measurable quantity. To do so, however, requires that one also record the ___X___. Otherwise, it is not possible to calculate moles. -CORRECT ANSWER-volume When working with gases, it is often necessary to use __ X __ as a measurable quantity. To do so, however, requires that one also record the ______. Otherwise, it is not possible to calculate moles. -CORRECT ANSWER-temperature and pressure When working at STP, Standard Pressure (1 atm or 101.325 kPa, or 760 mmHg) and Temperature (0oC, or 273.15 K), the ________ can be used to convert between liters and moles of an ideal gas. -CORRECT ANSWER-molar volume One mole of any ideal gas occupies _______ of space at STP. -CORRECT ANSWER-22.414L Aluminum reacts with hydrogen chloride to form aluminum chloride and hydrogen gas according to 2 Al(s) + 6 HCl(g) −−> 2 AlCl3(s) + 3 H2(g) Use equation stoichiometry and the molar volume of a gas to determine the volume of gas would be formed by reaction of 1.50 g Al(s) with excess HCl(g) at STP? -CORRECT ANSWER-1.87 L 1.50 g Al (1 mol Al / 26.98 g Al)(3 mol H2)(2 mol Al)(22.414 L / 1 mol H2) = 1.87 L Aluminum reacts with hydrogen chloride to form aluminum chloride and hydrogen gas according to 2 Al(s) + 6 HCl(g) → 2 AlCl3(s) + 3 H2(g) Use the Ideal Gas Constant, and then equation stoichiometry to determine how many kilograms of Al(s) will react with 525 L HCl(g) at 60.0 atm and 100 C? -CORRECT ANSWER-9.26 kg [Show More]

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