what mass, in grams, of calcium chloride dihydrate would she need to use to generate the 1.000 kg of caso₄…

what mass, in grams, of calcium chloride dihydrate would she need to use to generate the 1.000 kg of caso₄? molar mass caso₄ = 136.14 g/mol molar mass cacl₂·2h₂o = 147.01 g/mol znso₄·7h₂o + cacl₂·2h₂o → caso₄(s) + zncl₂ + 9h₂o ? g cacl₂·2h₂o

what mass, in grams, of calcium chloride dihydrate would she need to use to generate the 1.000 kg of caso₄? molar mass caso₄ = 136.14 g/mol molar mass cacl₂·2h₂o = 147.01 g/mol znso₄·7h₂o + cacl₂·2h₂o → caso₄(s) + zncl₂ + 9h₂o ? g cacl₂·2h₂o

Answer

Explanation:

Step1: Convert mass of ( \text{CaSO}_4 ) to moles

Given mass of ( \text{CaSO}_4 = 1.000 , \text{kg} = 1000 , \text{g} ), molar mass of ( \text{CaSO}_4 = 136.14 , \frac{\text{g}}{\text{mol}} ).
Moles of ( \text{CaSO}_4 = \frac{\text{mass}}{\text{molar mass}} = \frac{1000 , \text{g}}{136.14 , \frac{\text{g}}{\text{mol}}} \approx 7.345 , \text{mol} ).

Step2: Determine moles of ( \text{CaCl}_2 \cdot 2\text{H}_2\text{O} )

From the balanced equation, the mole ratio of ( \text{CaCl}_2 \cdot 2\text{H}_2\text{O} ) to ( \text{CaSO}_4 ) is ( 1:1 ). So moles of ( \text{CaCl}_2 \cdot 2\text{H}_2\text{O} = ) moles of ( \text{CaSO}_4 = 7.345 , \text{mol} ).

Step3: Calculate mass of ( \text{CaCl}_2 \cdot 2\text{H}_2\text{O} )

Molar mass of ( \text{CaCl}_2 \cdot 2\text{H}_2\text{O} = 147.01 , \frac{\text{g}}{\text{mol}} ).
Mass = moles ( \times ) molar mass = ( 7.345 , \text{mol} \times 147.01 , \frac{\text{g}}{\text{mol}} \approx 1079 , \text{g} ).

Answer:

( 1079 ) (or more precisely, using exact calculation: ( \frac{1000}{136.14} \times 147.01 \approx 1079 , \text{g} ))