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For the reaction 2x + 3y + 4z → 5w
Initially if 1 mole of x, 3 mole of y and 4 mole of z is taken. If 1.25 mole of w is obtained then % yield of this reaction is
Initially if 1 mole of x, 3 mole of y and 4 mole of z is taken. If 1.25 mole of w is obtained then % yield of this reaction is
- a)50%
- b)60%
- c)70%
- d)40%
Correct answer is option 'A'. Can you explain this answer?
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For the reaction 2x + 3y + 4z→ 5wInitially if 1 mole of x, 3 ...
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For the reaction 2x + 3y + 4z→ 5wInitially if 1 mole of x, 3 ...
Calculation of % yield:
1. Calculate the theoretical yield:
- Using the stoichiometry of the reaction, determine the moles of w that would be produced if all x, y, and z were completely converted.
- From the balanced equation, it can be seen that 2 moles of x, 3 moles of y, and 4 moles of z produce 5 moles of w.
- Therefore, if 1 mole of x, 3 moles of y, and 4 moles of z are reacted, the theoretical yield of w would be (5/2) moles.
2. Calculate the actual yield:
- Given that 1.25 moles of w are obtained, this is the actual yield of the reaction.
3. Calculate the % yield:
- % Yield = (Actual yield / Theoretical yield) x 100
- % Yield = (1.25 / (5/2)) x 100 = 50%
Therefore, the % yield of the reaction is 50%, which corresponds to option 'A'.
1. Calculate the theoretical yield:
- Using the stoichiometry of the reaction, determine the moles of w that would be produced if all x, y, and z were completely converted.
- From the balanced equation, it can be seen that 2 moles of x, 3 moles of y, and 4 moles of z produce 5 moles of w.
- Therefore, if 1 mole of x, 3 moles of y, and 4 moles of z are reacted, the theoretical yield of w would be (5/2) moles.
2. Calculate the actual yield:
- Given that 1.25 moles of w are obtained, this is the actual yield of the reaction.
3. Calculate the % yield:
- % Yield = (Actual yield / Theoretical yield) x 100
- % Yield = (1.25 / (5/2)) x 100 = 50%
Therefore, the % yield of the reaction is 50%, which corresponds to option 'A'.
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For the reaction 2x + 3y + 4z→ 5wInitially if 1 mole of x, 3 ...
2x + 3y + 4z = 5w
Moles 1 3 4
Stoichiometric coff. 2 1 1
Ratio 0.5 1 1
So, x is Limiting reagent.
So 0.5 = moles of w/5 (theoritical)
Or moles of w = 2.5
But obtained moles= 1.25
Therefore % yield = 1.25/2.5* 100 = 50%
Moles 1 3 4
Stoichiometric coff. 2 1 1
Ratio 0.5 1 1
So, x is Limiting reagent.
So 0.5 = moles of w/5 (theoritical)
Or moles of w = 2.5
But obtained moles= 1.25
Therefore % yield = 1.25/2.5* 100 = 50%
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For the reaction 2x + 3y + 4z→ 5wInitially if 1 mole of x, 3 mole of y and 4 mole of z is taken. If 1.25 mole of w is obtained then % yield of this reaction isa)50%b)60%c)70%d)40%Correct answer is option 'A'. Can you explain this answer?
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