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Standard XIII

Chemistry

Stoichiometry

Cl2 +2KOH → K...

Question

$C l_{2} + 2 K O H \to K C l + K C l O + H_{2} O$
$3 K C l O \to 2 K C l + K C l O_{3}$
$4 K C l O_{3} \to K C l + 3 K C l O_{4}$

2 moles of chlorine gas reacted with an excess of potassium hydroxide and 50 g of potassium perchlorate was obtained. Calculate the percentage yield of perchlorate in the reaction.
Molar mass of potassium perchlorate = 138.5 g/mol

72 %

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60 %

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90 %

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49 %

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Solution

The correct option is A 72 %
The complete balanced equation is:
$12 C l_{2} + 24 K O H \to 21 K C l + 3 K C l O_{4} + 12 H_{2} O$

12 moles of chlorine gives 3 moles of perchlorate.
2 moles of chlorine gives 0.5 moles of perchlorate.
Theoretical yield of perchlorate = 0.5 mole = 69.25 g
Experimental yield of perchlorate = 50 g
Percentage yield of perchlorate = $\frac{experimental yield}{theoretical yield} \times 100$ = $\frac{50 \times 100}{69.25} = 72$ %

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Similar questions

C l_{2} + 2 K O H \to K C l + K C l O + H_{2} O

3 K C l O \to 2 K C l + K C l O_{3}

4 K C l O_{3} \to K C l + 3 K C l O_{4}

2 moles of chlorine gas reacted with an excess of potassium hydroxide and 50 g of potassium perchlorate was obtained. Calculate the percentage yield of perchlorate in the reaction.
Molar mass of potassium perchlorate = 138.5 g/mol

Q. At STP 89.6 L of chlorine gas reacts with 560 g of

K O H

according to the following sequential reaction. Calculate the number of grams of

K C l O_{4}

. Molar mass of

K C l O_{4} = 138.5

g m o l^{- 1}

Molar mass of

K O H = 56

g m o l^{- 1}

C l_{2} + 2 K O H \to K C l + K C l O + H_{2} O

3 K C l O \to 2 K C l + K C l O_{3}

4 K C l O_{3} \to K C l + 3 K C l O_{4}

Q. From the following reaction sequence:

C l_{2} + 2 K O H \to K C l + K C l O + H_{2} O

3 K C l O \to 2 K C l + K C l O_{3}

4 K C l O_{3} \to 3 K C l O_{4} + K C l

Calculate the mass of chlorine that reacts with an excess of

K O H

needed to produce

100 g

K C l O_{4}

Q. From the following reaction sequence:

C l_{2} + 2 K O H \to K C l + K C l O + H_{2} O

3 K C l O \to 2 K C l + K C l O_{3}

4 K C l O_{3} \to 3 K C l O_{4} + K C l

Calculate the mass of chlorine that reacts with an excess of

K O H

needed to produce

100 g

K C l O_{4}

From the following reaction sequence
$C l_{2}$ + 2KOH $\to$ KCl + KClO + $H_{2} O$
3KClO $\to$ 2KCl + $K C l O_{3}$
$4 K C l O_{3}$ $\to$ $3 K C l O_{4} + K C l$

Calculate the mass of chlorine needed to produce 100g of $K C l O_{4}$

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Stoichiometry

Standard XIII Chemistry

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Cl2+2KOH→KCl+KClO+H2O 3KClO→2KCl+KClO3 4KClO3→KCl+3KClO4 2 moles of chlorine gas reacted with an excess of potassium hydroxide and 50 g of potassium perchlorate was obtained. Calculate the percentage yield of perchlorate in the reaction. Molar mass of potassium perchlorate = 138.5 g/mol