If standard enthalpy of vaporization of \(CCl_4\) is \(30.5\) kJ/mol, find heat absorbed for vaporization of \(294 \) gm of \(CCl_4\). [Nearest integer] [in kJ/mol]
If standard enthalpy of vaporization of \(CCl_4\) is \(30.5\) kJ/mol, find heat absorbed for vaporization of \(294 \) gm of \(CCl_4\). [Nearest integer] [in kJ/mol]
Correct Answer: 57
Solution and Explanation
Top Questions on Enthalpy change
- The bond dissociation energies of gaseous H2, Cl2, and HCl are 104, 58, and 103 kcal, respectively. The enthalpy of formation of HCl gas would be:
- BCECE - 2025
- Chemistry
- Enthalpy change
- What is the enthalpy of neutralization for CH3COOH + NaOH?
- BCECE - 2025
- Chemistry
- Enthalpy change
- The electron gain enthalpy (Cl2,H) of chlorine is -3.7 eV mol-1. How much energy (in kcal mol-1) is released when 71 g of chlorine atoms are completely converted into Cl- ions in gaseous state? (1 eV = 23 kcal)
- AP EAPCET - 2025
- Chemistry
- Enthalpy change
- Calculate the enthalpy change ($\Delta H$) for the combustion of 1 mole of methane ($\mathrm{CH}_4$) given the reaction: $$ \mathrm{CH}_4(g) + 2 \mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g) + 2 \mathrm{H}_2 \mathrm{O}(l) $$ Given bond energies: C–H = 413 kJ/mol, O=O = 498 kJ/mol, C=O = 803 kJ/mol, O–H = 467 kJ/mol.
- AP EAPCET - 2025
- Chemistry
- Enthalpy change
The enthalpy of combustion of methane is 890 kJ/mol. How much heat is released when 8 g of methane is burned completely? (Molar mass of CH\(_4\) = 16 g/mol)
- AP EAPCET - 2025
- Chemistry
- Enthalpy change
Questions Asked in JEE Main exam
Which of the following statement is true with respect to H\(_2\)O, NH\(_3\) and CH\(_4\)?
(A) The central atoms of all the molecules are sp\(^3\) hybridized.
(B) The H–O–H, H–N–H and H–C–H angles in the above molecules are 104.5°, 107.5° and 109.5° respectively.
(C) The increasing order of dipole moment is CH\(_4\)<NH\(_3\)<H\(_2\)O.
(D) Both H\(_2\)O and NH\(_3\) are Lewis acids and CH\(_4\) is a Lewis base.
(E) A solution of NH\(_3\) in H\(_2\)O is basic. In this solution NH\(_3\) and H\(_2\)O act as Lowry-Bronsted acid and base respectively.
- JEE Main - 2025
- Molecular Orbital Theory
- The increase in pressure required to decrease the volume of a water sample by 0.2percentage is \( P \times 10^5 \, \text{Nm}^{-2} \). Bulk modulus of water is \( 2.15 \times 10^9 \, \text{Nm}^{-2} \). The value of \( P \) is ________________.
- JEE Main - 2025
- System of Particles & Rotational Motion
The velocity-time graph of an object moving along a straight line is shown in the figure. What is the distance covered by the object between \( t = 0 \) to \( t = 4s \)?
- JEE Main - 2025
- Kinetic Energy
- Let \( P_n = \alpha^n + \beta^n \), \( P_{10} = 123 \), \( P_9 = 76 \), \( P_8 = 47 \), and \( P_1 = 1 \). The quadratic equation whose roots are \( \frac{1}{\alpha} \) and \( \frac{1}{\beta} \) is:
- JEE Main - 2025
- Sequences and Series
- The value of current \( I \) in the electrical circuit as given below, when the potential at \( A \) is equal to the potential at \( B \), will be ________________________ A.
- JEE Main - 2025
- Electrical Circuits
JEE Main Notification
GMC Azamgarh Admission 2025: Dates, Courses, Fees, Eligibility, SelectJuly 22, 2025Concepts Used:
Enthalpy change
Enthalpy Change refers to the difference between the heat content of the initial and final state of the reaction. Change in enthalpy can prove to be of great importance to find whether the reaction is exothermic or endothermic.
Formula for change in enthalpy is:-
dH = dU + d(PV)
The above equation can be written in the terms of initial and final states of the system which is defined below:
UF – UI = qP –p(VF – VI)
Or qP = (UF + pVF) – (UI + pVI)
Enthalpy (H) can be written as H= U + PV. Putting the value in the above equation, we obtained:
qP = HF – HI = ∆H
Hence, change in enthalpy ∆H = qP, referred to as the heat consumed at a constant pressure by the system. At constant pressure, we can also write,
∆H = ∆U + p∆V
Standard Enthalpy of Reaction
To specify the standard enthalpy of any reaction, it is calculated when all the components participating in the reaction i.e., the reactants and the products are in their standard form. Therefore the standard enthalpy of reaction is the enthalpy change that occurs in a system when a matter is transformed by a chemical reaction under standard conditions.