# Problem: Determine the limiting reactant (LR) and the mass (in grams) of ZnCl2 (molar mass = 136.3 g mol-1) that can be formed from 5.3 g of Zn and 7.4 g of HCl (molar mass = 36.5 g mol-1):Zn + 2 HCl → ZnCl2 + H2 A. LR = Zn; 6.17 g ZnCl2 formedB. LR = Zn; 11.05 g ZnCl2 formedC. LR = H2; 6.46 g ZnCl2 formedD. LR = HCl; 6.46 g ZnCl2 formedE. LR = HCl; 6.17 g ZnCl2 formed

###### FREE Expert Solution

Use stoichiometry and the balanced equation to determine which among Zn and HCl is the limiting reactant and the correct mass of ZnCl2 formed

For this matter, we need to find the molar mass of Zn. The molar mass of HCl and ZnCl2 is 36.5 g/mol and 136.3 g/mol

Zn            1 Zn × 65.38 g/mol Zn = 65.38 g/mol

88% (301 ratings) ###### Problem Details

Determine the limiting reactant (LR) and the mass (in grams) of ZnCl2 (molar mass = 136.3 g mol-1) that can be formed from 5.3 g of Zn and 7.4 g of HCl (molar mass = 36.5 g mol-1):

Zn + 2 HCl → ZnCl2 + H2

A. LR = Zn; 6.17 g ZnClformed

B. LR = Zn; 11.05 g ZnClformed

C. LR = H2; 6.46 g ZnClformed

D. LR = HCl; 6.46 g ZnClformed

E. LR = HCl; 6.17 g ZnClformed