The actual yield from the reaction is 92.4 grams.
What is percent yield?
Percent yield is the difference in the percent of theoretical yield to the percent of actual yield.
The balanced equation is
CaCO₃ + 2HCl → CaCl₂ + CO₂ + H₂O
Step 1- calculate the moles of CaCO₃
[tex]\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}\\\rm Number\;of \;moles= \dfrac{104 g}{100.08 g/mol} = 1.039 mol.[/tex]
The amount of CaCl₂ produced = no. of moles x molar mass
[tex](1.039 mol)\times (110.98 g/mol) = 114.3 g.[/tex]
Step2- calculate the percent yield
[tex]\rm percent\; yield = \dfrac{(actual\; yield)}{(theoretica\; yield)} \times 100\\\\\\\rm actual\; yield = \dfrac{(percent\; yield)\times (theoretica\; yield)}{100} \\\\\rm actual\; yield = \dfrac{(80.15)\times (115.3g)}{100} = 92.4 g[/tex]
Thus, the actual yield is 92.4 g.
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