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

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

Answer Link

Ondinne Ondinne · Answer 2 · 2019-10-16T00:36:42+02:00

Answer:

[tex]9.88gCaSO_{4}[/tex]

Explanation:

1. Find the balanced equation:

[tex]CaO+H_{2}SO_{4}=CaSO_{4}+H_{2}O[/tex]

2. Find the molecular weight of the [tex]CaSO_{4}[/tex]

Atomic weight of Ca = 40[tex]\frac{g}{mol}[/tex]

Atomic weight of S = 32[tex]\frac{g}{mol}[/tex]

Atomic weight of O = 16[tex]\frac{g}{mol}[/tex]

Molecular weight of [tex]CaSO_{4}[/tex] = 40 + 32 + (4*16)

Molecular weight of [tex]CaSO_{4}[/tex] = 136[tex]\frac{g}{mol}[/tex]

3. Use the stoichiometry to find the mass of [tex]CaSO_{4}[/tex] that can be produced:

[tex]4.070gCaO*\frac{1molCaO}{56gCaO}*\frac{1molCaSO_{4}}{1molCaO}*\frac{136gCaO}{1molCaSO_{4}}=9.88gCaSO_{4}[/tex]