wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

What mass of MnO2 is required to produce 1.12 litres of chlorine gas at STP acccording to the given equation?

MnO2 (s)+ 4HCl (aq)MnCl2 (aq)+ 2H2O (l)+ Cl2 (g)

Atomic masses of H = 1, Cl = 35.5, Mn = 55, O = 16

A
4.35 g
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
25.2 g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
6.1 g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
25.9 g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A 4.35 g
The molecular mass ofMnO2 = 55 + 32 = 87 g
Also, 1 mole of gas at STP acquires 22.4 litre volume.
The given equation is:

MnO2 (s)+ 4HCl (aq)MnCl2 (aq)+ 2H2O (l)+ Cl2 (g)

From the above equation, 1 mole of MnO2 is required to produce 1 mole of Cl2.

87 g of MnO2 is required to produce 22.4 L of Cl2 at STP

For 1.12 L of Cl2 = 1.12×8722.4 = 4.35 g ofMnO2 is required.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Mass Volume and Moles Relationship
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon