MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Ammonia

How much amou...

Question

How much amount of zinc is required to react with dilute $H_{2} S O_{4}$ for obtaining $224$ mL hydrogen at STP?

A

0.65

g

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

B

6.5

g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C

65

g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

0.065

g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $0.65$ g
$Z n + H_{2} S O_{4} \to Z n S O_{4} + H_{2}$
At STP 224 mL of hydrogen corresponds to $\frac{224}{1000 \times 22.4} = 0.01$ moles of hydrogen. They will be produced from the reaction of 0.01 mole of Zn with 0.01 mole of sulphuric acid. Hence, the mass of zinc required is $65.38 \times 0.01 = 0.65$ g.

Suggest Corrections

thumbs-up

0

Similar questions

Q. The amount of zinc required to produce

1.12 mL

H_{2}

at STP on treatment with

d i l . H C l

will be: (Given: Molar mass of

Z n

65 g / m o l

)

Q. The amount of zinc required to produce

224

H_{2}

at NTP on treatment with dilute

H_{2} S O_{4}

solution will be:

Q. The amount of zinc required to produce

1.12 mL

H_{2}

at STP on treatment with

d i l . H C l

will be: (Given: Molar mass of

Z n

65 g / m o l

)

Q. Amount of hydrogen produced when

H_{2} S O_{4}

reacts with 32.75 g of zinc is:

What volume of hydrogen measured at $27^{\circ} C$ and 776.7 mm pressure would be obtained by treating 0.65 g of pure zinc with sufficient amount of dilute hydrochloric acid? Aq. tension at $27^{\circ} C$ is 26.7 mm; At. mass of Zn is 65.

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Hydrides of Nitrogen - Ammonia and Hydrazine

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon