Question

calculate the mass of calcium sulfate that can be produced when 4.070g of calcium oxide react with excess sulfuric acid

Answer 1

`9.88gCaSO_(4)`

Step-by-step explanation:

1. Find the balanced equation:

`CaO+H_(2)SO_(4)=CaSO_(4)+H_(2)O`

2. Find the molecular weight of the
`CaSO_(4)`

Atomic weight of Ca = 40
`(g)/(mol)`

Atomic weight of S = 32
`(g)/(mol)`

Atomic weight of O = 16
`(g)/(mol)`

Molecular weight of
`CaSO_(4)` = 40 + 32 + (4*16)

Molecular weight of
`CaSO_(4)` = 136
`(g)/(mol)`

3. Use the stoichiometry to find the mass of
`CaSO_(4)` that can be produced:

`4.070gCaO*(1molCaO)/(56gCaO)*(1molCaSO_(4))/(1molCaO)*(136gCaO)/(1molCaSO_(4))=9.88gCaSO_(4)`

Answer 2

the chemical reaction to follow for this problem is :
CaO + H2SO4 --> CaSO4 + H2O

mass of CaSO4 = 4.07 g CaO ( 1 mol cao / 56 g cao ) ( 1 mol CaSO4 / 1 mol CaO) ( 136 g CaSO4 / 1 mol CaSO4 )

mass of CaSO4 = 9.88 g CaSO4