1)
Molar mass of H2SO4,
MM = 2*MM(H) + 1*MM(S) + 4*MM(O)
= 2*1.008 + 1*32.07 + 4*16.0
= 98.086 g/mol
mass(H2SO4)= 35.2 g
use:
number of mol of H2SO4,
n = mass of H2SO4/molar mass of H2SO4
=(35.2 g)/(98.09 g/mol)
= 0.3589 mol
Molar mass of Zn(OH)2,
MM = 1*MM(Zn) + 2*MM(O) + 2*MM(H)
= 1*65.38 + 2*16.0 + 2*1.008
= 99.396 g/mol
mass(Zn(OH)2)= 40.6 g
use:
number of mol of Zn(OH)2,
n = mass of Zn(OH)2/molar mass of Zn(OH)2
=(40.6 g)/(99.4 g/mol)
= 0.4085 mol
Balanced chemical equation is:
H2SO4 + Zn(OH)2 ---> ZnSO4 + 2 H2O
1 mol of H2SO4 reacts with 1 mol of Zn(OH)2
for 0.3589 mol of H2SO4, 0.3589 mol of Zn(OH)2 is required
But we have 0.4085 mol of Zn(OH)2
so, H2SO4 is limiting reagent
we will use H2SO4 in further calculation
Molar mass of ZnSO4,
MM = 1*MM(Zn) + 1*MM(S) + 4*MM(O)
= 1*65.38 + 1*32.07 + 4*16.0
= 161.45 g/mol
According to balanced equation
mol of ZnSO4 formed = (1/1)* moles of H2SO4
= (1/1)*0.3589
= 0.3589 mol
use:
mass of ZnSO4 = number of mol * molar mass
= 0.3589*1.614*10^2
= 57.94 g
Answer: 57.9 g
2)
H2SO4 is limiting reagent
Answer: H2SO4
3)
According to balanced equation
mol of Zn(OH)2 reacted = (1/1)* moles of H2SO4
= (1/1)*0.3589
= 0.3589 mol
mol of Zn(OH)2 remaining = mol initially present - mol reacted
mol of Zn(OH)2 remaining = 0.4085 - 0.3589
mol of Zn(OH)2 remaining = 4.96*10^-2 mol
Molar mass of Zn(OH)2,
MM = 1*MM(Zn) + 2*MM(O) + 2*MM(H)
= 1*65.38 + 2*16.0 + 2*1.008
= 99.396 g/mol
use:
mass of Zn(OH)2,
m = number of mol * molar mass
= 4.96*10^-2 mol * 99.4 g/mol
= 4.93 g
Answer: 4.93 g
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