qrxn is -8537.4 J
q/gram = -8537.4/0.47 = ?
q/mol = -8537.4/0.47g)*(24.3 g/mol) x (1 kJ/1000 J) = -441.4017 kJ/mol but if that 0.47 g Mg is correct you're allowed only two significant figures.
The answer for this question is ΔHrxn=-441.40174468085 kJ/mol but I don't know how to arrive to that answer.
0.47g of magnesium reacts with 100ml of 1.00 mol/L HCl in the following reaction: Mg(s)+2HCl(aq)-->MgCl2(aq)+H2(g). The heat of reaction is -8537.4J
Determine ΔHrxn.
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