Asked by Marty
A hydrate of zinc nitrate has the formula Zn(NO3)2 . xH2O. If the mass of 1 mol of anhydrous zinc nitrate is 63.67% of the mass of 1 mol of the hydrate, what is the value of x?
Answers
Answered by
DrBob222
So the %H2O = 100 - 63.67 = 36.33
a 100 g sample contains 64.67 g Zn(NO3)2 and 36.33 g H2O.
mols H2O = 36.33/18.015
mols Zn(NO3)2 = 63.67/molar mass zinc nitrate (don't include the water).
Find the ratio of mols H2O to 1 mol Zn(NO3)2. That will be x in the formula.
a 100 g sample contains 64.67 g Zn(NO3)2 and 36.33 g H2O.
mols H2O = 36.33/18.015
mols Zn(NO3)2 = 63.67/molar mass zinc nitrate (don't include the water).
Find the ratio of mols H2O to 1 mol Zn(NO3)2. That will be x in the formula.
Answered by
hamna
7.8
Answered by
Joe
x=6
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.