The net ionic equation of the reaction between Ksubscript2Crsubscript2Osubscript7 and FeSOsubscript4 in an acidic medium is given below:
Crsubscript2Osubscript7superscript2- + 6Fesuperscript2+ + 14H ---> 2Crsuperscript3+ 6Fesuperscript3+ +7H2O
a)how many moles of Ksubscript2Crsubscript2Osubscript7 can be reduced by 0.0865 mol of FeSOsubscript4?
b) how many moles of Crsuperscript3+ would be produced?
2007-09-08 07:34:36 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
1st; plz use better presentation to ur prob "don't use subscript".
2nd,the Sol:
the eq says:
Cr2O7(2-) + 6Fe(2+) + 14H ---> 2Cr(3+) + 6Fe(3+) + 7H2O
a)so the ratio bet Cr2O7 & Fe is 1:6 respectively.
so if 0.0865 is used in Fe so (1/6)(0.0865) moles of Cr2O7 so same no. of moles of K2Cr2O7 r used as 1 K2Cr2O7 gives 1 Cr2O7.
b)the ration bet the Cr2O7 & Cr is 1:2 as the eq says, so the no. of Cr moles is 2(1/6)(0.0865).
Use a calculator to calculate it.
2007-09-08 07:53:48 · answer #1 · answered by spidey 3 · 0⤊ 0⤋
a. 1/6 of 0.0865 moles.
b. 2/6 (=1/3) of 0.0865 moles.
Just use the numbers in front.
And don't bother writing subscript all the time!
2007-09-08 07:40:48 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋