Consider the following equation: Ag+ (aq) + CI-(aq) → Ag+CI- (s) ; ∆H = _65.7 kJmol-1. From the equation, it can be deduced that

Assessment: WAEC SSCE - Chemistry - 2001 (Objective) Subject: Chemistry

Question 1 Report

Consider the following equation: Ag⁺ _(aq) + CI-_(aq) → Ag⁺CI- _(s) ; ∆H = _65.7 kJmol^-1. From the equation, it can be deduced that

direct combination is involved and the reaction is endothermic

a solid is formed and heat is evolved

activation energy is high and a catalyst is required

the reaction is endothermic and occurs at high temperature

Answer Details

The given equation is a chemical equation that represents a reaction between silver ion (Ag⁺) and chloride ion (CI^-) to form silver chloride (Ag⁺CI^-). The value of enthalpy change (∆H) is given as -65.7 kJmol^-1, which indicates that the reaction is exothermic, i.e., heat is evolved during the reaction. Thus, the correct option is "a solid is formed and heat is evolved."

Read lesson note on Acids, Bases And Salts (Nigeria Only) (WAEC)

Acids, Bases And Salts (Nigeria Only)

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Consider the following equation: Ag+ (aq) + CI-(aq) → Ag+CI- (s) ; ∆H = _65.7 kJmol-1. From the equation, it can be deduced that

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