Exams › JEE Advanced › Chemistry
For the following reaction the equilibrium constant Kₑ at 298 K is 1.6 × 10¹⁷: Fe²⁺(aq) + S²⁻(aq) ⇌ FeS(s) When equal volumes of 0.06 M Fe²⁺(aq) and 0.2 M S²⁻(aq) solutions are mixed, the equilibrium concentration of Fe²⁺(aq) is found to be Y × 10⁻¹⁷ M. The value of Y is ____.
- 8
- 8.3
- 8.5
- 9
Correct answer: 8.3
Solution
The equilibrium constant is extremely large, indicating that almost all Fe²⁺ reacts to form FeS. Using the equilibrium expression and given concentrations, the remaining Fe²⁺ concentration is calculated to be 8.3 × 10⁻¹⁷ M.
Related JEE Advanced Chemistry questions
- K1, K2, and K3 represent the equilibrium constants for the following reactions, respectively: (I) \(N_2O_4 \rightleftharpoons 2NO_2\) (II) \(2NO_2 \rightleftharpoons N_2 + 2O_2\) (III) \(NO_2 \rightleftharpoons \tfrac{1}{2}N_2 + O_2\) Which of the following correctly describes the relationship between these constants?
- Which of the following sequences correctly represents the solubility order of the slightly soluble salts \(Hg_2Cl_2\), \(Cr_2(SO_4)_3\), \(BaSO_4\), and \(CrCl_3\)?
- For the decomposition of ammonium carbamate according to the reaction \(NH_2COONH_4(s) \rightleftharpoons 2NH_3(g) + CO_2(g)\), the equilibrium constant \(K_p\) is \(2.9 \times 10^{-2}\,\text{atm}^3\). If 1 mole of \(NH_2COONH_4\) is initially present, what is the total pressure at equilibrium?
- In which of the following cases can the pH be determined using the equilibrium constant(s) provided?
- In the equilibrium reaction \(NH_2COONH_4(s) \rightleftharpoons 2NH_3(g) + CO_2(g)\), which change will cause the partial pressure of \(NH_3\) to rise?
- For the reaction \(XY_2(g) \rightleftharpoons XY(g) + Y(g)\), if the degree of dissociation \(\alpha\) is very small compared to 1, how is \(\alpha\) related to the pressure \(P\)?
⚔️ Practice JEE Advanced Chemistry free + battle 1v1 →