Exams › JEE Main › Chemistry
2O3(g) ⇌ 3O2(g) At 300 K, ozone is fifty percent dissociated. The standard free energy change at this temperature and 1 atm pressure is ________ J mol−1. (Nearest integer) [Given: ln 1.35 = 0.3 and R = 8.3 J K−1 mol−1]
- 747.00
- 747.00
- 747.00
- 747.00
Correct answer: 747.00
Solution
The standard free energy change can be calculated using the relationship between the equilibrium constant and free energy. Given that ozone is fifty percent dissociated, the equilibrium constant can be determined, and applying the formula ΔG° = -RT ln K leads to the calculated value of 747.00 J mol−1.
Related JEE Main Chemistry questions
- The solubility product constants of Ag$_2$CrO$_4$, AgCl, AgBr and AgI are $1.1\times10^{-12}$, $1.8\times10^{-10}$, $5.0\times10^{-13}$ and $8.3\times10^{-17}$, respectively. If AgNO$_3$ solution is added to a mixture containing equal amounts of NaCl, NaBr, NaI and Na$_2$CrO$_4$, which silver salt will begin to precipitate at the highest Ag$^+$ concentration, i.e. the last one to form?
- Two sparingly soluble salts, MY and NY$_3$, each have the same solubility product constant, $K_{sp}=6.2\times10^{-13}$, at room temperature. Which of the following statements is correct for these two salts?
- Given the equilibrium constants for these reactions: $\text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3$, $K_1$ $\text{N}_2 + \text{O}_2 \rightleftharpoons 2\text{NO}$, $K_2$ $\text{H}_2 + \tfrac12\text{O}_2 \rightleftharpoons \text{H}_2\text{O}$, $K_3$ What is the equilibrium constant $K$ for the reaction $2\text{NH}_3 + \tfrac52\text{O}_2 \rightleftharpoons 2\text{NO} + 3\text{H}_2\text{O}$?
- In a saturated solution of Ag$_2$C$_2$O$_4$, the concentration of Ag$^+$ ions is $2.2\times10^{-4}\ \text{mol L}^{-1}$. The solubility product constant, $K_{sp}$, of Ag$_2$C$_2$O$_4$ is:
- Which species can behave as both a Brønsted acid and a Brønsted base?
- Select the correct statement: Polyphosphates are used as water-softening agents because they
⚔️ Practice JEE Main Chemistry free + battle 1v1 →