metallic zinc reacts with aqueous HCL. Zn (s) + 2HCL(aq)---> ZnCl 2 (aq)+ H2 (g)

Question

metallic zinc reacts with aqueous HCL.

Zn (s) + 2HCL(aq)---> ZnCl 2 (aq)+ H2 (g)

what volume of 2.5M HCL, in milliliters, is required to convert 12.9 G of Zn completely to products?

INTERACTIVE EXAMPLE Stoichiometry of a Reaction in Solution Metallic zinc reacts with aqueous HCL Zn(s)-2 HCl(aq) ZnCl2(aq) + H2(g) What volume of 2.50 M HCI in milliters, is required to convert 12.9 g of Zn completely to products? mL HCI X show Approach Show Tutor Steps Submit Answer Try Another Verslon 2 item attempts remaining

Explanation / Answer

Zn (s) + 2HCL(aq)---> ZnCl 2 (aq)+ H2 (g)

no of moles of Zn   = W/G.A.Wt

                               = 12.9/65.4   = 0.197 moles

from balanced equation

1 mole of Zn react with 2 moles of HCl

0.197 moles of Zn react with = 2*0.197/1   = 0.394moles of HCl

no of moles of HCl = molarity * volume in L

0.394                      = 2.5*volume in L

volume in L              = 0.394/2.5   = 0.1576L   = 157.6ml of HCl >>>>answer

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