Cl + e ----> Cl- ΔH = -348kJ/mol The value -348KJ/mol in this case will be:
Correct answer: C. Electron affinity
- A. Ionization energy
- B. Electronegativity
- C. Electron affinity
- D. Entropy
- E. Free energy
Explanation
As it can be seen in the equation, electrons are gained by the element chlorine to form a negative ion (anion). The process in which electrons are gained is called electron affinity.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Thermochemistry and Energetics of Chemical Reactions
Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
Practise Thermochemistry and Energetics of Chemical Reactions
728 free Thermochemistry and Energetics of Chemical Reactions MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Thermochemistry and Energetics of Chemical Reactions questions
The measurement of heat absorbed or given out in a chemical reaction is referred to as:
Transfer of heat from hot surroundings to a cold refrigerator is an example of:
Hydrogen is a diatomic molecule and its molecule have
For a reaction given below C(s) + O2 (g) -> CO2 (g) + 394 kJ / mol The enthalpy of reaction is
For a chemical reaction A -> B, the threshold energy of the reaction is 37 kJ/mole. The average internal energy of A is 12 kJ/Mole. What will be the activation energy of A?
Two rocket fuels below are determined by their high performance. N2H4(l) + O2(g) -> N2(g) + 2H2O(l) ΔH= -632 kJ H2 (g) + ½ O2(g) -> H2O(l) ΔH = -286 kJ If equal masses of hydrazine and hydrogen are used, which of the following has better performance?