wiz-icon
MyQuestionIcon
MyQuestionIcon
2
You visited us 2 times! Enjoying our articles? Unlock Full Access!
Question

Phosphoric acid (H3PO4) is prepared in a two-step process:
(1) P4+5O2P4O10
(2) P4O10+6H2O4H3PO4
In step (1), 62 g of phosphorus is made to react with excess oxygen to form P4O10 with 85 % yield. In step (2), the yield of H3PO4 obtained is 90 %. Calculate the mass of H3PO4 produced.

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

The correct option is B 150 g
P4+5O2P4O10.(1)
P4O10+6H2O4H3PO4.(2)
Moles of P4=62124=0.5 mol
In reaction 1,
1 mol of P4 produces 1 mol of P4O10
0.5 mol of P4 will produce 0.5 mol of P4O10
Yield of the reaction is given as 85 %
Moles of P4O10 formed =0.85×0.5=0.425 mol
In reaction 2,
1 mol of P4O10 produces 4 mol of H3PO4
0.425 mol will produce (4×0.425)=1.7 mol of H3PO4
Yield of the reaction is given as 90 %
Moles of H3PO4 formed =1.7×0.9=1.53 mol
Mass of H3PO4 formed =98×1.53=150 g

flag
Suggest Corrections
thumbs-up
1
similar_icon
Similar questions
View More
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Stoichiometric Calculations
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon