Given the following balanced equation, select all statement(s) that is/are True.

Question

Given the following balanced equation,

2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g)  ∆H_rxn = −368.4 kJ

Select all statement(s) that is/are True.

Group of answer choices

A. The temperature of the solution increases when the reaction is carried out in a coffee-cup calorimeter.

B. The heat associated for reacting 1 mol H₂O(l) is −184.2 kJ.

C. The reaction is endothermic.

D. The heat associated for the reaction of  2 NaOH(aq) + H2(g)→2 Na(s) + 2 H₂O(l) is +368.4 kJ.

Answer 1

A. The temperature of the solution increases when the reaction is carried out in a coffee-cup calorimeter. True because the ∆H is negative meaning heat is given off by the reaction

B. The heat associated for reacting 1 mol H₂O(l) is −184.2 kJ. True b/c it would be half of what it is for 2 moles

C. The reaction is endothermic. False. The reaction is exothermic as indicated by the negative value of ∆H

D. The heat associated for the reaction of  2 NaOH(aq) + H2(g)→2 Na(s) + 2 H₂O(l) is +368.4 kJ. False. The heat of that reaction would be +368.4 kJ