Consider 0.022 grams of h2(g) produced by following chemical reaction, 2HCI(aq) +Mg(s)---->Cl2(aq)+H2(g)

Question

True or False

1)The reaction requires 0.795 grams of HCI(aq)

2)The reaction also produces 1.04 grams of MgCl2(aq)

3) the number of moles of the reactants consumed will equal the number of moles of the products made

Answer 1

Reaction is 2HCl(aq) + Mg(s) ==> MgCl2(aq) + H2(g)

Given: 0.022 g of H2(g) are produced

FInd: moles of H2 gas.

0.022 g H2 x 1 mol H2/2 g = 0.011 moles H2 gas

FInd moles HCl needed:

0.011 mol H2 x 2 mol HCl/ mol H2 = 0.022 mol HCl needed

Find mass HCl needed:

0.022 mol HCl x 36.5 g /mol = 0.803 g HCl needed - SO #1 IS FALSE

Find moles Mg(s) needed:

0.011 mol H2 x 1 mol Mg / mol H2 = 0.011 mol Mg needed

Find mass of MgCl2 produced:

0.011 mol H2 x 1 mol MgCl2 / mol H2 = 0.011 mol MgCl2 produced

Find mass of MgCl2 produced:

0.011 mol MgCl2 x 95.2 g/mol = 1.05 g MgCl2 produced - SO #2 IS TRUE

moles of reactants = 0.022 HCl + 0.011 Mg = 0.033 moles

moles products = 0.011 H2 + 0.011 MgCl2 = 0.022 moles

SO #3 IS FALSE