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

Verified Answer :

taskmasters

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

Ondinne

Answer:

\(9.88gCaSO_{4}\)

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\(\frac{g}{mol}\)

Atomic weight of S = 32\(\frac{g}{mol}\)

Atomic weight of O = 16\(\frac{g}{mol}\)

Molecular weight of \(CaSO_{4}\) = 40 + 32 + (4*16)

Molecular weight of \(CaSO_{4}\) = 136\(\frac{g}{mol}\)

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

\(4.070gCaO*\frac{1molCaO}{56gCaO}*\frac{1molCaSO_{4}}{1molCaO}*\frac{136gCaO}{1molCaSO_{4}}=9.88gCaSO_{4}\)

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