1.10.0 g of sodium bicarbonate, NaHCO3(s) (MW 84.01 g/mol) is reacted with an ex
ID: 1042011 • Letter: 1
Question
1.10.0 g of sodium bicarbonate, NaHCO3(s) (MW 84.01 g/mol) is reacted with an excess of hydrochloric acid, at a constant pressure of 1 atm, according to the following reaction: NaHCO;(s) + HCl(aq)-NaCl(a) +H)+Co (2) Calculate the amount of heat absorbed/evolved in this reaction. AH 28.3 k 2. From the following entahlpies of reaction: C(s) +02(g) CO2(g_... AH--394 kJ 2H2(g) + O2(g) ?2H2O(l) M_-572 kJ Use Hess' Law to calculate AH for the reaction: 2C(s) +3H2(g CHg) 3. If you heat magnesium carbonate (MW 84.32 g/mol) sufficiently it will decompose to give magnesium oxide and carbon dioxide. According to the following balanced thermochemical equation: MiKX);() .?. Miy(Xs):KXh(v) ALI 117.3 kJ 567 g of magnesium carbonate. seExplanation / Answer
1.
Mass of NaHCO3 = 10;0 g.
Molar mass of NaHCO3 = 84.01 g/mol
Moles of NaHCO3 = mass / molar mass = 10.0 / 84.01 = 0.119 mol
From the balacned equation
1 mol of NaHCO3 on reaction with HCl needs 28.3 kJ
Then, 0.119 mol of NaHCO3 needs 0.119 * 28.3 = 3.37 kJ of heat
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