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0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is?
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0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at S...
Calculation of Volume of H2 Evolved from Reaction of 0.9g Al with Dil. HCl at STP
Given:
Mass of Al (m) = 0.9g
Molar Mass of Al (M) = 27g/mol
2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
The balanced chemical equation shows that 3 moles of H2 are produced for every 2 moles of Al reacted.
Calculations:
1. Moles of Al reacted = m/M = 0.9/27 = 0.0333 mol
2. Moles of H2 produced = 3/2 x 0.0333 = 0.05 mol
3. Volume of H2 at STP = (22.4 L/mol) x 0.05 mol = 1.12 L
Explanation:
The given problem is a stoichiometry problem that requires the use of the balanced chemical equation to determine the moles of H2 produced from the reaction of 0.9g Al with dilute HCl. The balanced chemical equation shows that 3 moles of H2 are produced for every 2 moles of Al reacted. Therefore, the first step is to calculate the moles of Al reacted using its mass and molar mass.
Once the moles of Al reacted are known, the moles of H2 produced can be determined using the mole ratio from the balanced chemical equation. Finally, the volume of H2 at STP can be calculated using the molar volume of a gas (22.4 L/mol) and the number of moles of H2 produced.
Conclusion:
The volume of H2 evolved from the reaction of 0.9g Al with dilute HCl at STP is 1.12 L.
Given:
Mass of Al (m) = 0.9g
Molar Mass of Al (M) = 27g/mol
2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
The balanced chemical equation shows that 3 moles of H2 are produced for every 2 moles of Al reacted.
Calculations:
1. Moles of Al reacted = m/M = 0.9/27 = 0.0333 mol
2. Moles of H2 produced = 3/2 x 0.0333 = 0.05 mol
3. Volume of H2 at STP = (22.4 L/mol) x 0.05 mol = 1.12 L
Explanation:
The given problem is a stoichiometry problem that requires the use of the balanced chemical equation to determine the moles of H2 produced from the reaction of 0.9g Al with dilute HCl. The balanced chemical equation shows that 3 moles of H2 are produced for every 2 moles of Al reacted. Therefore, the first step is to calculate the moles of Al reacted using its mass and molar mass.
Once the moles of Al reacted are known, the moles of H2 produced can be determined using the mole ratio from the balanced chemical equation. Finally, the volume of H2 at STP can be calculated using the molar volume of a gas (22.4 L/mol) and the number of moles of H2 produced.
Conclusion:
The volume of H2 evolved from the reaction of 0.9g Al with dilute HCl at STP is 1.12 L.
Community Answer
0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at S...
1.12 liters maybe
tell me is it right or not
tell me is it right or not
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0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is?
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0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is?.
0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 0.9g Al reacts with dil. HCL to give H2. The volume of H2 evolved at STP is?.
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