CHEMICAL EQUILIBRIUM

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CHEMICAL EQUILIBRIUM

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On addition of ammonium chloride to a solution of ammonium hydroxide: 

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An acidic buffer solution can be prepared by mixing:

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Aqueous solutions of HNO3 , KOH, CH3COOH, and CH3COONa of identical concentrations are provided. The pairs(s) of solutions which form at buffer upon mixing is (are):

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The species present in solution when CO dissolved in water are: 

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In some solutions, the concentration of H3O+ remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as:

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The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is: 

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1M NaCl and IM HCl are present in an aqueous solution. The solution is: 

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At infinite dilution, the percentage ionization for both strong and weak electrolyte is:

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NaOH is a strong base because: 

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The pH of 0.1 M solution of the following salts increases in the order: 

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The pH of a solution is increased from 3 to 6, its H+ ion concentration will be:

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The pH of a 10^–9 M solution of HCl in water is:

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An aqueous solution of sodium carbonate is alkaline because sodium carbonate is a salt of:

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The pKa for acid A is greater than pKa for acid B. The strong acid is:

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The number of H+ ions present in 1 cm³ of a solution whose pH is 10 is:

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An aqueous solution of ammonia consists of:

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An aqueous solution of ammonia consists of:

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Which of the following statements is not true? 

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Which of the following is the strongest acid?

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Which anion is the weakest base?

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What would be the pH of H3PO4 if it loses two protons in aqueous solution?

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The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of this acid is: 

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Ionic product in water increases if:

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The degree of ionization of a compound depends on: 

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Molten sodium chloride conducts electricity due to the presence of:

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Which of the following can act both as a Bronsted acid and a Bronsted base? 

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Strength of an acid can be explained on the basis of:

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Which of the following is the strongest acid?

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Out of which of the following pair of acids, the first one is more acidic?

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The conjugate base of hydrazoic acid is:

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The decomposition of N2O4 at 25°C, N2O4(g)   2NO2 has KC=4.61 x 10^–3 . A 2.00 dm^3 vessel contained 0.0466 mol NO, at equilibrium. What was the concentration of NO₂ in the vessel?

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The equilibrium constant Kc for the reaction N₂+ 3H2 2NH3 is 0.5 dm^6 mol^-1 at 400 K. Find  Kp. given that R=0.0821 atm dm^3 K^-1 mol^-1:

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For the reaction CO(g) + Cl2(g) COCl2(g) the ratio Kp/KC is equal to:

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In which of the following reaction, the value of Kp will be equal to Kc

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The thermal dissociation equilibrium of CaCO3(s) is studied under different conditions = CaCO3(s)   CaO(s) + CO2(g). For this equilibrium, the incorrect statement(s) is (are): 

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The following equilibrium exists in aqueous solution CH3COOH CH3COO+ H+ If dil. HCl is  added without change in temperature, the:

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In presence of a catalyst, what happens to the chemical equilibrium? 

(I) Energy of activation of the forward and reverse reactions is lowered by the same amount. 

(II) Equilibrium amount is not disturbed. 

(III) Rates of forward and reverse reaction increase by the same factor. 

(IV) More product is formed 

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Consider the reaction equilibrium, 2SO2(g)+ O2(g)  ⇌  2SO3(g) with △H^0= -198 kJ. On the basis of Le Chatelier's principle, the conditions. favourable for forward reaction is:

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The increase of pressure on ice water system at constant temperature will lead to:

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What happens when an inert gas is added to an equilibrium keeping volume unchanged? 

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Which change will increase the equilibrium concentration of SO3?

 2SO2(g) + O2(g) 2SO3(g) + heat

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"If a system is subjected to stress, the system acts to relieve the effects of the stress" Who proposed this idea?

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How does a catalyst speed up a chemical reaction? 

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The equilibrium constant at 1300K for the reaction H2+Br2(g) 2HBr(g) is 1.6×10^5. What is the value of Kc for the reverse reaction?

45 / 87

What affects the numerical value of the equilibrium constant for a reversible reaction at equilibrium?

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For the reaction, 2NO2(g) N2O4(g) which value of the equilibrium constant indicates the largest concentration of NO2

47 / 87

According to Le Chatelier's principle, which chemical system shifts to the right when pressure is increased?

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Basic buffer is prepared by mixing together a weak base, and its salt with: 

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In a gas phase reaction, if the number of moles of reactants are equal to the number of moles of product, then:

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The equilibrium constant for a reaction 2O3 3O2 is 10^55 at 25°C, it tells that ozone is:

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In an exothermic reversible reaction, the equilibrium will shift towards the forward direction by:

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The rate at which a reaction precedes is directly proportional to the product of active masses of reactants. This is:

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When HCl is passed in saturated solution of NaCl, the solubility of NaCl is:

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The strongest acid among halogen acids is:

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The pH of 10 moles/dm³ of Ba(OH): is:

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Which aqueous solution has highest pH? 

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The pH of 10-2 moles dm-3 of an aqueous solution of HCl is: 

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Catalyst used in preparation of NH3 from N2 and H2 is: 

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The relationship between Kp and Kc is given by:

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The units of Kc for reaction N₂+O22NO will be: 

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Which relationship is correct about the strength an acid with the strength of its conjugated base?

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The aqueous solution of BiCl3 is cloudy. Cloudiness of BiCl3 solution can be cleared by:

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In case when [OH-]> [H+] the solution is:

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Equilibrium constant for gaseous equilibrium is represented by:

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Ionization of hydrogen sulphide gas is suppressed by: 

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Concentrations of reactants and products at equilibrium are:

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By adding NH4Cl to NH4OH solution, the ionization of NH4OH:

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High value of Ka means that acid is:

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In Haber process, for formation of NH3 the pressure used is:

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If NaOH is added to a solution of CH3COOH then:

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The law of mass action was given by:

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Molar concentration is called:

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A large value of Kc means that at equilibrium:

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The ionic product of water will increase if: 

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A basic buffer solution can be prepared by mixing:

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The suppression of ionization of weak acid or a weak base by adding one of its own ions is: 

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Strength of an acid is determined from the value of:

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In which of the following reactions, Kc and Kp will be equal: 

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Catalyst used in preparation of SO3 gas from SO2 is:

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The units of Kc for the reaction of ammonia synthesis are:

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The units for Kw of H2O are:

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Sum of pH and pOH at 25°C is always equal to:

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Optimum temperature for synthesis of ammonia by Haber process is:

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Which one affects the value of Kc?

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When Kc value of a reaction is very small, the equilibrium position lies to:

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The value of Kw of water at 25°C is:

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The pH of a solution is 9, the solution is: 

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