3. Which gaseous product(s) in the above reactions is (are) flammable? 4. Consid

Question

3. Which gaseous product(s) in the above reactions is (are) flammable? 4. Consider the balanced equation for the reaction of magnesium metal with hydrochloric acid. (a) Calculate the minimum number of moles of HCl required for the reaction of each gram of magnesium metal. Show all work. Write balanced equations for the reaction of the three solids listed in the experiment's materials list (Mg, CaCOs, NazCOs)with aqueous hydrochloric acid. Include physical states. 2. 3. Which gascous product(s) in the above reactions is (are) flammable? 1 Consider the balanced equation for the reaction of magnesium metal with hydrochloric acid. , (a) Calculate the minimum number of moles of HCI required for the reaction of each gram of magnesium metal. Show all work

Explanation / Answer

Q2

All these reacitons are decopmosition reactions

will form gases:

Mg(s) + 2HCl(aq) --> H2(g) + MgCl2(aq)

CaCO3(s) + 2HCl(aq) --> CaCl2(aq) + H2O(l) + CO2(g)

Na2CO3(s) + 2HCl(aq) --> 2NaCl(aq) + H2O(l) + CO2(g)

Q3

CO2 is already oxidized, so only H2(g) will be flammable

choose Mg + Hcl

Q4

min. mol of HCl per 1 g of Mg

1 g = change to mol

mol = mass/MW = 1/24.3 = 0.04115

1 mol of Mg = 2 mol of HCl

0.04115 mol --> 2*0.04115 = 0.0823 mol of HCl

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