Chemical - Phase - Ionic Equilibriums - Chemistry MCQ

The number of degrees of freedom in the homogenous liquid region of a two component system with a eutectic point, at one atmosphere pressure is:

The maximum number of triple point(s) occuring in one component sulfur system are:           

Choose correct:           

Consider the following equilibrium in a closed vessel  . At a fixed temperature if the volume of the reaction vessel is halved, which of the following statements holds true regarding the equilibrium constant (K_p) and the degree of dissociation (α) of N₂O₄?

Under conditions of constant temperature and pressure when a system is in equilibrium which of the following quantities is at a minimum:           

Based upon the following hypothetical equilibrium at 273 K

Which is the most effective dehydrating agent at 273 K (Aqueous tension at 273 K = 6.0 × 10^–3atm)

An equilibrium system for the reaction between hydrogen and iodine to give hydrogen iodine at 765 K in a 5 liter volume contains 0.4 mole of hydrogen, 0.4 mole of iodine and 2.4 moles of hydrogen iodide. The equilibrium constant for the reaction is:

To a 50 ml of 0.1 M HCl solution, 10 ml of 0.1 M NaOH is added and the resulting solution is diluted to 100 ml. What is change in pH of the HCl solution?           

To a 100 ml solution of 0.1 M CH₃COONa and 0.1 M CH₃COOH, 0.4 gm of solid NaOH was added. Assuming volume remains constant, calculate the change in pH value? Given that pK_a(CH₃COOH) = 4.74.           

When equal volumes of the following solution are mixed, precipitation of AgCl (K_sp = 1.8 × 10^–10) will occur only with:​

How many gram of CaC₂O₄ will dissolve in one litre of saturated solution? K_sp of CaC₂O₄ is 2.5 × 10^–9mol^–2 and its molecular weight is 128:           

Let the solubilities of AgCl in H₂O, 0.01 M CaCl₂; 0.01 M NaCl and 0.05 M AgNO₃ be S₁, S₂, S₃, S₄ respectively. What is the correct relationship between these quantities?           

 Calculate the minimum mole % of CO₂ in air at 1 bar which is sufficient to prevent any loss in weight of Ag₂CO₃ by decomposition at the same temperature:

At temperature T, a compound AB₂(g) dissociates according to the reaction  with degree of dissociation α, which is small compared with unity. The expression for K_p, in terms of α and the total pressure, P_T is:

A reaction mixture containing H₂, N₂ and NH₃ has partial pressures 2 atm, 1 atm and 3 atm respectively at 725 K. If the value of Kp for the reaction.  is4.28 × 10^–5atm^–2 at 725 K, in which direction the net reaction will go:           

pH of an aqueous solution of Al⁺³ is likely to be:           

The molar solubility (in mol L^–1) of a sparingly soluble salt MX₄ is ‘s’. The corresponding solubility product is K_sp. s is given in terms of K_sp by the relation:

The phase diagram of a pure substance is sketched below:

The number of degrees of freedom at points P1, P2 and P3, respectively, are:

Consider a phase diagram of two component simple eutectic system. If X_A = 0.8 and X_B = 0.2, which of the following composition will never be observed:           

The number of phases, components and degrees of freedom, when Ar is added to an equilibrium mixture of NO, O₂ and NO₂ in gas phase are, respectively:           

A pure substance exists in several different phases A, B, C. Its partial phase diagram is shown below: 
          
Which of the following statements is correct about the above diagram?           

The lowest pressure at which the liquid phase of a pure substance can exist is known as:           

The solid-liquid phase diagram for the Mg-Zn system is shown in the figure below where the vertical line at X(Mg) = 0.33 represents the formation of a congruent melting compound MgZn₂.The figure is divided into seven regions depending upon the physical state of the system. The composition of the region #6 represents.

Which of the following does not represent a phase diagram?

For the reaction  the degree of dissociation (α) of HI(g) is related to equilibrium constant K_p by the expression:

Choose correct:          

Solid CO₂ is called ‘dry ice’ because: