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

A 0.60g sample consisting of only CaC2O4 and MgC2O4 is heated at 500C, converting the two salts of CaCO3 and MgCO3. The sample then, weighs 0.465g. If the sample had been heated to 900C, where the products are CaO and MgO, what would the mixtures of oxides have weighed?

A
0.12g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
0.21g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
0.252g
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
0.3g
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is C 0.252g
Let xg is the weight of CaC2O4 and (0.6x) g be the weight of MgC2O4.

The reactions are as follows:
CaC2O4CaCO3+CO2
MgC2O4MgCO3+CO2

Weight of CaCO3 produced=x128×100.
Weight of MgCO3 produced=(0.6x)112×84.

x128×100+(0.6x)112×84=0.465.

Therefore, x=0.48g

Due to further heating,
CaCO3CaO+CO2

- x128

MgCO3MgO+CO2

- 0.6x112

Weight of CaO and MgO produced =0.48128×56+0.12112×40=0.252g.

Hence, option C is correct.

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