JEE Exam > JEE Questions > The combustion of benzene (1) gives CO2(g) an...
Start Learning for Free
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :
- a)4152.6
- b)-452.46
- c)3260
- d)-3267.6
Correct answer is option 'D'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Verified Answer
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat...
Most Upvoted Answer
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat...
Given:
The combustion of benzene (1) gives CO2(g) and H2O(I).
Heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250°C.
To find:
Heat of combustion of benzene at constant pressure.
Solution:
1. Understanding the concept:
The heat of combustion at constant volume is the energy released when a substance is burned completely under constant volume conditions.
The heat of combustion at constant pressure is the energy released when a substance is burned completely under constant pressure conditions.
Since the combustion of benzene is happening in an open container, it is safe to assume that it is happening at constant pressure.
2. Applying the concept:
The heat of combustion at constant volume can be related to the heat of combustion at constant pressure using the equation:
ΔHcombustion = ΔHconstant volume + ΔnRT
Where:
ΔHcombustion = Heat of combustion at constant pressure
ΔHconstant volume = Heat of combustion at constant volume
Δn = Change in the number of moles of gas
R = Ideal gas constant
T = Temperature in Kelvin
3. Calculating the change in the number of moles of gas:
The combustion of benzene produces 6 moles of gas (CO2) and 3 moles of liquid (H2O). Therefore, the change in the number of moles of gas (Δn) is 6.
4. Converting temperature to Kelvin:
The given temperature is 250°C. To convert it to Kelvin, we add 273.15 to the Celsius temperature. Therefore, the temperature in Kelvin is 523.15 K.
5. Calculating the heat of combustion at constant pressure:
Using the equation mentioned in step 2, we have:
ΔHcombustion = ΔHconstant volume + ΔnRT
Plugging in the values, we get:
ΔHcombustion = -3263.9 kJ mol-1 + (6 moles * 8.314 J mol-1 K-1 * 523.15 K)
Calculating this expression, we get -3267.6 kJ mol-1.
Answer:
The heat of combustion of benzene at constant pressure is -3267.6 kJ mol-1, which is option 'D'.
The combustion of benzene (1) gives CO2(g) and H2O(I).
Heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250°C.
To find:
Heat of combustion of benzene at constant pressure.
Solution:
1. Understanding the concept:
The heat of combustion at constant volume is the energy released when a substance is burned completely under constant volume conditions.
The heat of combustion at constant pressure is the energy released when a substance is burned completely under constant pressure conditions.
Since the combustion of benzene is happening in an open container, it is safe to assume that it is happening at constant pressure.
2. Applying the concept:
The heat of combustion at constant volume can be related to the heat of combustion at constant pressure using the equation:
ΔHcombustion = ΔHconstant volume + ΔnRT
Where:
ΔHcombustion = Heat of combustion at constant pressure
ΔHconstant volume = Heat of combustion at constant volume
Δn = Change in the number of moles of gas
R = Ideal gas constant
T = Temperature in Kelvin
3. Calculating the change in the number of moles of gas:
The combustion of benzene produces 6 moles of gas (CO2) and 3 moles of liquid (H2O). Therefore, the change in the number of moles of gas (Δn) is 6.
4. Converting temperature to Kelvin:
The given temperature is 250°C. To convert it to Kelvin, we add 273.15 to the Celsius temperature. Therefore, the temperature in Kelvin is 523.15 K.
5. Calculating the heat of combustion at constant pressure:
Using the equation mentioned in step 2, we have:
ΔHcombustion = ΔHconstant volume + ΔnRT
Plugging in the values, we get:
ΔHcombustion = -3263.9 kJ mol-1 + (6 moles * 8.314 J mol-1 K-1 * 523.15 K)
Calculating this expression, we get -3267.6 kJ mol-1.
Answer:
The heat of combustion of benzene at constant pressure is -3267.6 kJ mol-1, which is option 'D'.
Attention JEE Students!
To make sure you are not studying endlessly, EduRev has designed JEE study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in JEE.
|
Explore Courses for JEE exam
|
|
Similar JEE Doubts
Top Courses for JEEView all
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer?
Question Description
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer?.
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer?.
Solutions for The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.
Here you can find the meaning of The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer?, a detailed solution for The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice The combustion of benzene (1) gives CO2(g) and H2O(I). Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol-1 at 250 C; heat of combust ion (in kJ mol-1) of benzene at constant pressure will be :a)4152.6b)-452.46c)3260d)-3267.6Correct answer is option 'D'. Can you explain this answer? tests, examples and also practice JEE tests.
|
|
Explore Courses for JEE exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup