wiz-icon
MyQuestionIcon
MyQuestionIcon
8
You visited us 8 times! Enjoying our articles? Unlock Full Access!
Question

In the laboratory a student was determining the formula for the hydrate of barium chloride, BaCl2. The student cleaned, dried and determined the mass of the crucible and cover. The student then added a sample of the hydrate to the crucible and determined the mass. The student heated the sample in the crucible strongly for 10 minutes. The sample in the crucible and cover was cooled and the mass was determined. The mass data is provided in the table below:

Mass of crucible and cover31.623 grams
Mass of crucible, cover, and sample prior to heating33.632 grams
Mass of crucible, cover, and sample after heating33.376 grams
After the heating, how many moles of water were removed from the sample?

A
0.0142 moles
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
0.0974 moles
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
0.112 moles
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
0.256 moles
No worries! We‘ve got your back. Try BYJU‘S free classes today!
E
1.85 moles
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is C 0.0142 moles
Mass of the crucible, cover and the hydrated sample before heating was 33.632grams
Mass of the crucible, cover and the sample after heating was 33.376grams
Clearly, some amount of water has already evaporated.
Amount of water removed is (33.63233.376) grams that is 0.256grams
Molecular weight of water is 18grams
18grams of water is equivalent to 1mole
1gramof water is equivalent to 118mole
0.256grams of water is equivalent to 118×0.256mole that is equal to 0.0142moles
Option A is the correct answer.

flag
Suggest Corrections
thumbs-up
0
similar_icon
Similar questions
View More
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Percentage Composition and Molecular Formula
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon