BITSAT Equilibrium — practice questions
32 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice BITSAT Equilibrium in the app →For the homogeneous gas-phase reaction $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$ at equilibriumLe Chatelier's principle says that if a system at equilibrium is disturbed, the system will shift in the direcFor the synthesis of ammonia $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, increasing the pressure on the syAt a certain temperature, the equilibrium constant $K_c$ for $A \rightleftharpoons B$ is $4$. If the initial cFor the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$, the relationship between $K_p$ and $K_c$ is:At $25°C$, the ionic product of water $K_w = [H^+][OH^-] = 10^{-14}$. What is the pH of pure water at $25°C$?For the reaction aA + bB ⇌ cC + dD at equilibrium, the equilibrium constant Kc is:For an exothermic reaction at equilibrium, increasing temperature will shift the equilibrium:Le Chatelier's principle states that a system at equilibrium responds to a stress by:For the reaction N2 + 3H2 ⇌ 2NH3, increasing pressure favours:Equilibrium constant of a reaction is INDEPENDENT of:Relation between Kp and Kc for a gas reaction with Δn_gas = change in moles of gas:For an endothermic reaction, increasing T shifts equilibrium:For dissociation of weak acid HA in water: HA ⇌ H+ + A-. Equilibrium constant is called:pH of a 0.01 M HCl solution:pOH of a solution with pH = 8.5 (at 25°C):Solubility product Ksp of AgCl is 1.6 × 10⁻¹⁰. Its solubility in pure water (mol/L):For a buffer solution containing weak acid HA and its salt NaA, the pH is approximately:At equilibrium for an exothermic reaction, increasing pressure (for gas reaction with Δn < 0):At 500 K, Kc for N2 + 3H2 ⇌ 2NH3 is 60 (in mol⁻² L²). Kp at 500 K (R = 0.0821):For weak acid HA with Ka = 10⁻⁵, [H+] in 0.1 M solution is approximately:Buffer capacity is maximum when:A weak base BOH has Kb = 1.8 × 10⁻⁵. pH of 0.1 M solution is approximately:Solubility of CaF2 in water (Ksp = 4.0 × 10⁻¹¹):For the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g), if initial pressure of PCl5 is P0 and degree of dissociation is αFor the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), at equilibrium increasing pressure:If K = 1 for a reaction, the standard free energy change ΔG°:At 298 K, water has Kw = 10⁻¹⁴. Concentration of H+ in pure water:At equilibrium, the ratio of forward to reverse reaction rates:In a saturated solution of AgCl, [Ag+] = 1.26 × 10⁻⁵. If KNO3 is added (no common ion), solubility of AgCl:For the reaction H2(g) + I2(g) ⇌ 2HI(g) with Kc = 50 at 800 K, if [H2] = [I2] = 0.01 M initially, equilibrium Degree of dissociation α of weak acid HA (Ka = 1.8 × 10⁻⁵) in 0.01 M solution: