Asked by Jade
C6H6(l) + Cl2(g) --> C6Cl6(s) + HCl(g)
Consider the unbalanced equation above. What is the maximum mass of each of the products that can be formed when 72.5 g of C6H6 and 49.0 g Cl2 react?
Consider the unbalanced equation above. What is the maximum mass of each of the products that can be formed when 72.5 g of C6H6 and 49.0 g Cl2 react?
Answers
Answered by
DrBob222
1. Balance the equation.
2a Convert 72.5 g C6H6 to moles. mol = g/molar mass
2b. Do the same for 49.0g Cl2.
3a. Using the coefficients in the balanced equation, convert moles C6H6 to moles of the product.
3b. Do the same for Cl2.
3c. You will get two different answers; obviously both can't be right. The correct answer to choose in limiting reagent problems is ALWAYS the smaller value and the reagent providing that number is the limiting reagent.
4. Using the smaller number of mols, convert to grams. g = mols x molar mass.
2a Convert 72.5 g C6H6 to moles. mol = g/molar mass
2b. Do the same for 49.0g Cl2.
3a. Using the coefficients in the balanced equation, convert moles C6H6 to moles of the product.
3b. Do the same for Cl2.
3c. You will get two different answers; obviously both can't be right. The correct answer to choose in limiting reagent problems is ALWAYS the smaller value and the reagent providing that number is the limiting reagent.
4. Using the smaller number of mols, convert to grams. g = mols x molar mass.
Answered by
Niki
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