11th Standard CBSE Syllabus & Materials

11th Standard CBSE

CBSE 11th Economics PART-A - Presentation of Data - New Sample Question Papers Study Material - QB365 Set A

NEW

11th Standard CBSE

CBSE 11th Economics PART-A - Organisation of Data - New Sample Question Papers Study Material - QB365 Set A

NEW

11th Standard CBSE

CBSE 11th Economics PART-A - Collection of Data - New Sample Question Papers Study Material - QB365 Set A

NEW

11th Standard CBSE

CBSE 11th Economics PART-A - Introduction to Economics and Statistics - New Sample Question Papers Study Material - QB365 Set A

NEW

11th Standard CBSE

CBSE 11th Business Studies International Trade Sample Question Papers Study Material - QB365 Set A

NEW

11th Standard CBSE

CBSE 11th Business Studies Evolution and Fundamentals of Business Sample Question Papers Study Material - QB365 Set A

CBSE 11th Standard Chemistry Subject Thermodynamics Ncert Exemplar 1 Mark Questions With Solution 2021

Published on: 27/05/2021

QB365 Provides the updated NCERT Exemplar Questions for Class
11, and also provide the detail solution for each and every NCERT
Exemplar questions. NCERT Exemplar questions are latest updated
question pattern from NCERT, QB365 will helps to get more marks in Exams

Download CBSE Class 11th Standard CBSE Chemistry question papers, sample papers, important questions, and previous year solved papers in PDF format. Get free study materials, NCERT solutions, and exam preparation resources for Class 11th Standard CBSE Chemistry

Questions + Answers key

Take MCQ Chemistry Test

QB365 Student Learing Managemnet System

Std: 11th Standard CBSE - Chemistry

chapter: - NCERT Exemplers

Visit QB365-SLMS - https://www.qb365.in/slms/ Complete Questions and Answers

Questions:

Generic 2

5 x 2 = 10

At 298 K, K_p for the reaction, N₂O₄(g) \(\leftrightharpoons \) 2NO₂(g) is 0.98. Predict whether the reaction is spontaneous or not.

Which quantity out of \(\Delta _{ r }G\) and \(\Delta _{ r }G^{ \circ }\) will be zero at equilibrium?

The enthalpy of atomisation for the reaction,
\({ CH }_{ 4 }\left( g \right) \longrightarrow C\left( g \right) +4H\left( g \right) \)
is 1665 KJ mol^-1. What is the bond energy of C-H bond ?

Given that \(\Delta H\) = 0 for mixing of two gases. Explain whether the diffusion of these gases into each other in a closed container is a spontaneous process or not?

Enthalpy of combustion of carbon to CO₂ is –393.5 kJ mol^–1. Calculate the heat released upon formation of 35.2 g of CO₂ from carbon and dioxygen gas.

Visit QB365-SLMS - https://www.qb365.in/slms/

Answers Key:

Generic 2

5 x 2 = 10

Δ_rG^∘= −2.303 RT logK_p
Here K_p= 0.98, i.e. K_p < 1 therefore, Δ_rG^∘ is positive. Hence, the reaction is non-spontaneous.

\(\Delta_r G=\Delta_r G^{\circ}+R T \ln K\)
At equilibrium,
\( 0=\Delta_r G^{\circ}+R T \ln K\left(\because \Delta_r G=0\right) \)
\( \text { or } \Delta_r G^{\circ}=-R T \ln K \)
\(\Delta_r G^{\circ}=0 \text { when } K=1\)
For all other values of \(\mathrm{K}, \Delta_r G^{\circ}\) will be non-zero.

In CH₄ there are four C-H bonds. The enthalpy of atomisation of 1 mole of CH₄ means dissociation of four moles of C-H bond.
∴ C-H bond energy per mol \(=\frac{ 1665 KJ}{4 mol }\)= 416.25 KJ mol^-1.

It is a spontaneous process because although ΔH=0, i.e., energy factor has no role to play but randomness increases, i.e. randomness factor favours the process.

The reaction for the combustion of carbon into CO₂ is
C(s) + O₂(g) ⟶ CO₂(g); △H = -393.5 KJ mol^-1
Heat released in the formation of 44 g CO₂ = 393.5 KJ
∴∴ Heat released in the formation of 35.2 g CO₂
\(=\frac{393 KJ × 35.2 g}{44 g} \)= 314.8 KJ