C(s) + H2O(g) → H2(g) + CO2(g) ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is

Assessment: JAMB UTME - Chemistry - 2009 Subject: Chemistry

Question 1 Report

C(s) + H2O(g) → H2(g) + CO2(g)

ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is

not feasible

at equilibrium

feasible

exothermic

Answer Details

At 1300K, the value of ΔG for the given reaction is negative (-43KJ), indicating that the reaction is feasible. A negative ΔG value implies that the products are more stable than the reactants, and the reaction will proceed spontaneously in the forward direction. The fact that ΔG is negative also means that the reaction is exothermic, releasing energy to the surroundings. Therefore, the correct answers are: feasible and exothermic.

Read lesson note on Kinetic Theory Of Matter And Gas Laws (JAMB)

Kinetic Theory Of Matter And Gas Laws

View Answer

C(s) + H2O(g) → H2(g) + CO2(g) ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is

Related Questions

Download The App On Google Playstore