Consider the following reaction:
2Na + Cl2(g) → 2NaCl ΔH = -821.8 kJ
(a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced during an enthalpy change of 16.5 kJ? (d) How many kilojoules of heat are absorbed when 44.1 g of NaCl is decomposed into Na and Cl2 at constant pressure?
a.
dH is -. By definition that is exothermic.
b.
You get 821.8 kJ for 2*23 or 46 g Na. So 5.6 g Na will give you
821..8 kJ x 5.6/46 = ? kJ.
c.
Rearrange part b. You have 821.8 kJ when 2*58.5 g NaCl are formed.
So 2*58.5 g NaCl x 16.5 kJ/821.8 kJ = ?
d.
See b and c parts.
How do I solve this? Na(s) + Cl2(9) + 2NaCl(s), AH = -821.8 kJ (a) Is this reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 8.0 g of Na(s) reacts according to this reaction at constant pressure. (c) How many grams of NaCl are produced during an enthalpy change of 10.0 kJ? (d) How many kJ of heat are absorbed when 25.0 g of NaCl(s) is decomposed into Na(s) and Cl2(9) at constant pressure?
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