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What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:
- a)44.8 L
- b)22.4 L
- c)89.6 L
- d)67.2 L
Correct answer is option 'D'. Can you explain this answer?
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What volume of hydrogen gas at 273 K and 1 atm pressure will be consum...
Calculation of Volume of Hydrogen Gas Consumed in Obtaining Elemental Boron
Given:
Amount of boron (B) obtained = 21.6 g
Atomic mass of boron (B) = 10.8
Pressure (P) = 1 atm
Temperature (T) = 273 K
We can use the balanced chemical equation for the reduction of boron trichloride (BCl3) with hydrogen (H2) to obtain elemental boron (B):
BCl3 + 3H2 → B + 3HCl
From the equation, we can see that one mole of boron is obtained by reacting 3 moles of hydrogen gas. Therefore, we can use the following steps to calculate the volume of hydrogen gas consumed:
Step 1: Calculate the number of moles of boron obtained
Number of moles of B = Mass of B / Atomic mass of B
Number of moles of B = 21.6 g / 10.8 g/mol
Number of moles of B = 2 mol
Step 2: Calculate the number of moles of hydrogen gas required
From the balanced equation, we know that 3 moles of H2 react with 1 mole of B. Therefore, the number of moles of H2 required is:
Number of moles of H2 = 3 x Number of moles of B
Number of moles of H2 = 3 x 2 mol
Number of moles of H2 = 6 mol
Step 3: Calculate the volume of hydrogen gas consumed
Using the ideal gas law, we can calculate the volume of hydrogen gas consumed:
PV = nRT
where:
P = Pressure = 1 atm
V = Volume of H2
n = Number of moles of H2 = 6 mol
R = Gas constant = 0.0821 L atm mol^-1 K^-1
T = Temperature = 273 K
Rearranging the equation, we get:
V = nRT / P
V = 6 mol x 0.0821 L atm mol^-1 K^-1 x 273 K / 1 atm
V = 134.52 L
Therefore, the volume of hydrogen gas consumed in obtaining 21.6 g of elemental boron is 134.52 L. However, the question asks for the volume of hydrogen gas at STP (standard temperature and pressure), which is 0°C (273 K) and 1 atm. At STP, one mole of any ideal gas occupies 22.4 L. Therefore, we need to convert the volume of hydrogen gas at the given conditions to STP:
Volume of H2 at STP = (134.52 L / 6 mol) x (1 mol / 22.4 L)
Volume of H2 at STP = 1.20 L/mol x 6 mol
Volume of H2 at STP = 7.20 L
Therefore, the volume of hydrogen gas at STP consumed in obtaining 21.6 g of elemental boron is 7.20 L, which is option (d) in the given choices.
Given:
Amount of boron (B) obtained = 21.6 g
Atomic mass of boron (B) = 10.8
Pressure (P) = 1 atm
Temperature (T) = 273 K
We can use the balanced chemical equation for the reduction of boron trichloride (BCl3) with hydrogen (H2) to obtain elemental boron (B):
BCl3 + 3H2 → B + 3HCl
From the equation, we can see that one mole of boron is obtained by reacting 3 moles of hydrogen gas. Therefore, we can use the following steps to calculate the volume of hydrogen gas consumed:
Step 1: Calculate the number of moles of boron obtained
Number of moles of B = Mass of B / Atomic mass of B
Number of moles of B = 21.6 g / 10.8 g/mol
Number of moles of B = 2 mol
Step 2: Calculate the number of moles of hydrogen gas required
From the balanced equation, we know that 3 moles of H2 react with 1 mole of B. Therefore, the number of moles of H2 required is:
Number of moles of H2 = 3 x Number of moles of B
Number of moles of H2 = 3 x 2 mol
Number of moles of H2 = 6 mol
Step 3: Calculate the volume of hydrogen gas consumed
Using the ideal gas law, we can calculate the volume of hydrogen gas consumed:
PV = nRT
where:
P = Pressure = 1 atm
V = Volume of H2
n = Number of moles of H2 = 6 mol
R = Gas constant = 0.0821 L atm mol^-1 K^-1
T = Temperature = 273 K
Rearranging the equation, we get:
V = nRT / P
V = 6 mol x 0.0821 L atm mol^-1 K^-1 x 273 K / 1 atm
V = 134.52 L
Therefore, the volume of hydrogen gas consumed in obtaining 21.6 g of elemental boron is 134.52 L. However, the question asks for the volume of hydrogen gas at STP (standard temperature and pressure), which is 0°C (273 K) and 1 atm. At STP, one mole of any ideal gas occupies 22.4 L. Therefore, we need to convert the volume of hydrogen gas at the given conditions to STP:
Volume of H2 at STP = (134.52 L / 6 mol) x (1 mol / 22.4 L)
Volume of H2 at STP = 1.20 L/mol x 6 mol
Volume of H2 at STP = 7.20 L
Therefore, the volume of hydrogen gas at STP consumed in obtaining 21.6 g of elemental boron is 7.20 L, which is option (d) in the given choices.
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What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer?
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What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer?.
What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (at. mass = 10.8) from the reduction of boron trichloride with hydrogen:a)44.8 Lb)22.4 Lc)89.6 Ld)67.2 LCorrect answer is option 'D'. Can you explain this answer?.
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