From the following reaction sequenceCl2 - 2KOH - KCl - KClO - H2 O3KClO - 2KCl - KClO34KClO3 - 3KClO4 - KClCalculate the mass of chlorine needed to produce 23g of KClO4

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Concentration Terms - An Introduction (w/w etc)

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Question

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 23g of $K C l O_{4}$

142g

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35.5g

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248.5g

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215.5g

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Solution

The correct option is A
142g

The given reactions involve certain compounds which are not needed for calculations.
$∴$ Balance the reaction in a way that the unnecessary compounds get cancelled.
$12 C l_{2}$ + 24KOH $\to$ 12KClO + 12KCl + $12 H_{2} O$
12KClO $\to$ 8KCl + $4 K C l O_{3}$
$4 K C I O_{3}$ $\to$ $3 K C l O_{4}$ + KCl
$12 C l_{2}$ + 24KOH $\to$ $3 K C l O_{4}$ + 21KCl + $12 H_{2} O$
We cancel the compounds on either side of the arrow
From this final balanced equation
12 moles of $C l_{2}$ gives 3 moles of $K C l O_{4}$
12 $\times$ (35.5 $\times$ 2=71)g = 3 $\times$ (138.5)g
$∴ 23 g o f K C I O_{4} = \frac{23 \times 12 \times 71}{3 \times 138.5}$

$23 g o f K C l O_{4}$ gives $\approx 142 g o f C l_{2}$

Note: approximate weight of $K C l O_{4} \approx= 138$

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Similar questions

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 23g of $K C l O_{4}$

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}

K C l O_{4}

is obtained from the following sequence of reactions:

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}

.

The correct statement among the following is/are

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}

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From the following reaction sequence Cl2 + 2KOH → KCl + KClO + H2O 3KClO → 2KCl + KClO3 4KClO3 → 3KClO4+KCl Calculate the mass of chlorine needed to produce 23g of KClO4

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 23g of $K C l O_{4}$