The positive change in enthalpy occurs in (1) II2( g)+(1)/(2) O2( g) ⟶II2( g) (2) N2( g)+3 II2(

Name: Problem 13, Chapter 6: Objective Chemistry for Engineering and Medical Entrance Examinations
Uploaded: 2022-01-25T07:44:18-08:00
Duration: 35 s
Channel: Mishal Gul
Description: The positive change in enthalpy occurs in (1) II2( g)+(1)/(2) O2( g) ⟶II2( g) (2) N2( g)+3 II2( g) ⟶2 NII3( g) (3) MgCO3( s) ⟶MgO(s)+CO2( g) (4) H2( g)+(1)/(2) O2( g) ⟶H2 O(I)

step 1 The positive change in enthalpy occurs. There are 4 types of chemical reactions given. Out of th

Question

The positive change in enthalpy occurs in (1) $\mathrm{II}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{II}_{2}(\mathrm{~g})$ (2) $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{II}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NII}_{3}(\mathrm{~g})$ (3) $\mathrm{MgCO}_{3}(\mathrm{~s}) \longrightarrow \mathrm{MgO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ (4) $\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})$

   The positive change in enthalpy occurs in
(1) $\mathrm{II}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{II}_{2}(\mathrm{~g})$
(2) $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{II}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NII}_{3}(\mathrm{~g})$
(3) $\mathrm{MgCO}_{3}(\mathrm{~s}) \longrightarrow \mathrm{MgO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$
(4) $\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})$

Objective Chemistry for Engineering and Medical Entrance Examinations

K Rama Rao 1st Edition

Chapter 6, Problem 13

Instant Answer

Solved by Expert Mishal Gul

01/25/2022

Step 1

In this reaction, solid magnesium carbonate is decomposing into solid magnesium oxide and carbon dioxide gas. Show more…

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The positive change in enthalpy occurs in (1) $\mathrm{II}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{II}_{2}(\mathrm{~g})$ (2) $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{II}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NII}_{3}(\mathrm{~g})$ (3) $\mathrm{MgCO}_{3}(\mathrm{~s}) \longrightarrow \mathrm{MgO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ (4) $\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{I})$

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Key Concepts

Enthalpy Change

Enthalpy change is the heat absorbed or released under constant pressure during a chemical reaction. A positive enthalpy change indicates that the reaction absorbs heat from the surroundings, making it endothermic, whereas a negative change indicates that heat is released, making the reaction exothermic.

Endothermic and Exothermic Reactions

Chemical reactions can either absorb energy (endothermic) or release energy (exothermic). In endothermic reactions, the system takes in heat, resulting in a positive change in enthalpy, which is often necessary for processes such as decomposition. In contrast, exothermic reactions release energy, resulting in a negative enthalpy change.

Decomposition Reactions

Decomposition reactions typically require an input of energy to break chemical bonds in a compound, which often makes them endothermic. The energy absorbed in breaking bonds during the process is reflected in a positive enthalpy change.

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