If 9.00 grams of Cr(ClO4)3 are mixed with 4.00 grams of K2CO3, how much reactant is left over?
K2CO3 + Cr(ClO4)3
this is double replacement:
Cr(CLO4)3 + K2CO3 = KCLO4 + Cr2(CO3)3
balanced:
2 Cr(CLO4)3 + 3 K2CO3 = 6 KCLO4 + Cr2(CO3)3
mol of Cr(ClO4)3 = mass/MW = 9 / 350.3479 = 0.025688
mol of K2CO3 = mass/MW = 4 /284.0189 = 0.0140835
then
ratio is
2:3
0.025688 need 3/2
1.5*0.025688 = 0.038532 mol of K2CO3 bu we only have 0.0140835
thjerefore
this ilimiting
0.0140835*2/3 = 0.009389mol of CrClo43 reacted
then
0.025688-0.009389 = 0.016299 mol of f Cr(ClO4)3 mol
mass = mol*MW = 350.3479*0.016299 = 5.71032 g
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