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Standard XII

Chemistry

Potassium Permanganate

Consider the ...

Question

Consider the reaction:
$2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}$
This reaction has an $80.0$ yield.
What mass of $Z n O$ is produced when $50.0 g Z n S$ is heated in an open vessel untill no further weight loss is observed?

33.4 g

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40.4 g

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43.4 g

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3240 g

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Solution

The correct option is C $33.4 g$
Molar mass of $Z n S = 97.5 g$
No. of moles of $Z n O = \frac{50}{97.5} = 0.5128 m o l e s$
$2 m o l e s$ of $Z n S$ produce $2 m o l e s$ of $Z n O .$
So, $0.5128 m o l e s$ produce $0.5128 m o l e s$ of $Z n O .$
So, mass of $Z n O = (0.5128) \times 81 = 41 g$
As percentage yield $= 80 %$
$\Rightarrow$ Mass of $Z n O = \frac{80}{100} \times 41 = 33.4 g$

Suggest Corrections

Similar questions

Consider following reactions:

(a) $2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}$

$Z n O + C \to Z n + C O$

(b)

2 Z n S + C \to 2 Z n + C S_{2}

Which reaction has more positive value of

Δ G

?
1. A
2. B
3. A and B are same
4. None

Q. The reaction

2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}

in the metallurgical process of zinc is called

2 Z n + O_{2} ⟶ 2 Z n O; Δ G^{o} = - 616 J . . (i)

2 Z n + 2 S ⟶ 2 Z n S; Δ G^{o} = - 293 J . . . (i i)

2 S + 2 O_{2} ⟶ 2 S O_{2} (g); Δ G^{o} = - 408 J . . (i i i)

Δ G^{o}

for the following reaction:

2 Z n S + 3 O_{2} ⟶ 2 Z n O + 2 {S O}_{2}

would be:

The chief ore of

Z n

is the sulphide,

Z n S

. The ore is concentrated by froth floatation process and then heated in air to convert

Z n S

Z n O

2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}

(

75 %

conversion)

Z n O + H_{2} S O_{4} \to Z n S O_{4} + H_{2} O

(

100 %

conversion )

2 Z n S O_{4} + 2 H_{2} O \to 2 Z n + 2 H_{2} S O_{4} + O_{2}

(

80 %

conversion)

The mass of

Z n

obtained from a sample of ore containing

292.2

kg of

Z n S

will be :

Q. Following method of extracting

Z n

is based on thermodynamics
A :

2 Z n S + 3 O_{2} ⟶ 2 Z n O + 2 S O_{2}

B :

Z n O + C ⟶ Z n + C O

△ G_{f}^{o}

(standard free energies of formation, in

k J m o l^{- 1}

) of

Z n S = - 205.4, Z n O = - 318.0, S O_{2} = - 300.4

and of

C O = - 137.3

Free energy changes of the above reaction A and B (respectively) will be :

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Consider the reaction:2ZnS+3O2→2ZnO+2SO2This reaction has an 80.0 yield.What mass of ZnO is produced when 50.0 g ZnS is heated in an open vessel untill no further weight loss is observed?

The correct option is C 33.4 gMolar mass of ZnS=97.5 gNo. of moles of ZnO=5097.5=0.5128 moles2 moles of ZnS produce 2 moles of ZnO.So, 0.5128 moles produce 0.5128 moles of ZnO.So, mass of ZnO=(0.5128)×81=41 gAs percentage yield =80%⇒ Mass of ZnO=80100×41=33.4 g

Consider the reaction:
$2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}$
This reaction has an $80.0$ yield.
What mass of $Z n O$ is produced when $50.0 g Z n S$ is heated in an open vessel untill no further weight loss is observed?