Q71E
Question
Outline the steps needed to determine the limiting reactant when 0.50 mol of Cr and 0.75 mol of H3PO4 react according to the following chemical equation. \(2Cr + 2{H_3}P{O_4} \to 2CrP{O_4} + 3{H_2}\). Determine the limiting reactant.
Step-by-Step Solution
Verified Answer
Cr is the limiting reactant.
1Determine the number of moles
Find the number of moles of \({H_3}P{O_4}\).
Mol \({H_3}P{O_4} = 0.50\,mol\,Cr\,\left( {\frac{{2\,mol\,{H_3}P{O_4}}}{{2\,mol\,Cr}}} \right) = 0.50\,mol\,{H_3}P{O_4}\).
2Determine the limiting reactant
Only 0.50 mol of \({H_3}P{O_4}\)is required but we have 0.75 mol of \({H_3}P{O_4}\) so, \({H_3}P{O_4}\)is in excess amount. Thus, Cr is the limiting reactant.
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