27 g of silver was reacted with excess sulfur, according to the following equation: 2Ag+S→Ag2S 25 g of silver sulfide was collected. What are the theoretical yield, actual yield, and percent yield?
A
31 g, 35 g, 71%
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
21 g , 33 g , 69%
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
31 g, 25 g, 81%
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
31 g, 45 g, 91%
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution
The correct option is C31 g, 25 g, 81% 2Ag+S→Ag2S The atomic mass of Ag and S are 108 g/mol and 32 g/mol respectively.
The Molar mass of Ag2S=2(108)+32=248 g/mol. 2 moles of Ag gives 1 mole of Ag2S. 27 g of Ag will give 27108×2×248=31 of Ag2S. Hence, the theoretical yield is 31 g. However only 25 g of silver sulfide was collected. Hence, the actual yield is 25 g. The percentage yield is 25×10031=81 %.