Tiêu đề 8. Chemical Eq Med.pdf ✅

1.)Which of the following is an example of homogeneous equilibrium? (a.) 2SO2(g) + O2(g) 2SO3(g) (b.) C(s) + H2O(g) CO(g) + H2(g) (c.) CaCO3(s) CaO(s) +CO2(g) (d.) NH4HS(s) NH3(g) + H2S(g) 2.)For the reaction : 2(g) 2(g) H + I 2HI(g) , the standard free energy is G 0. o   The equilibrium constant (K) would be. (a.) K = 0 (b.) K > 1 (c.) K = 1 (d.) K < 1 3.)For the reaction, 2SO2(g) + O2(g) 2SO3(g) what is Kc when the equilibrium concentration of [SO2 ] = 0.60M,[O2 ] = 0.82 M and [SO3 ] =1.90 M ? (a.) 1 12.229Lmol− (b.) 1 24.5 L mol− (c.) 1 36.0 Lmol− (d.) 3 1 2.67 10 Lmol−  4.)Which of the following is not a general characteristiec of equilibria involving physical processes? (a.) Equilibrium is possible only in a closed system at a given temperature. (b.) The equilibrium is dynamic in nature. (c.) Measurable poroperties of the system keep changing. (d.) Equilibrium can be attained from both sides of the reaction. 5.)A reaction is said to be in equilibrium when (a.) The rate of transformation of reactants to products is equal to the rate of transformation of products to the reactants (b.) 50% of the reactants are converted to products (c.) The reaction is near completion and all the reactants are converted to products (d.) The volume of reactants is just equal to the volume of the products. 6.)What is observed at equilibrium point in the reaction? PCls(g) PCl3(g) +Cl 2(g) (a.) Equal volumes of 5 PCl3 PCl , and Cl 2 are present. (b.) Equal masses of 5 PCl3 PCl , and Cl 2 are present. (c.) The concentrations of PCl5, PCl3 and Cl 2 become constant. (d.) Reaction comes to a stop. 7.)Which of the following is not true about a reversible reaction? (a.) The reaction does not proceed to completion. (b.) It cannot be influenced by a catalyst. (c.) Number of moles of reactants and products is always equal. (d.) It can be attained only in a closed container. 8.)Consider the following graph and mark the correct statement.
(a.) Chemical equilibrium in the reaction, 2 2 H + I 2HI can be attained from either directions. (b.) Equilibrium can be obtained when H2 and 2 I are mixed in an open vessel. (c.) The concentrations of H2 and 2 I keep decreasing while concentration of HI keeps increasing with time. (d.) We can find out equilibrium concentration of H2 and 2 I from the given graph. 9.)If the equilibrium constant for the given reaction is 0.25 No O , 2 1 N 2 1 2 + 2 then the equilibrium constant for the reaction 2 O2 2 1 N 2 1 + No will be (a.) 1 (b.) 2 (c.) 3 (d.) 4 10.)If the equilibrium constant for the reaction. 2XY X2 + Y2 is 81, What is the value of equilibrium constant for the reaction. XY 2 Y2 2 1 X 2 1 + (a.) 81 (b.) 9 (c.) 6561 (d.) 40.5 11.)If the value of equilibrium constant Kc for the reaction, N2 + 3H2 2NH3 is 7. The equilibrium constant for the reaction 2N2 + 6H2 4NH3 will be (a.) 49 (b.) 7 (c.) 14 (d.) 28 12.)At 473, K, Kc for the reaction PCl5(g) PCl3(g) +Cl 2(g) is 3 8.3 10−  . What will be the value of Kc for the formation of PCl5 at the same temperature? (a.) 3 8.310 (b.) 120.48 (c.) 3 8.3 10−  (d.) 240.8 13.)The value of Kc for the following equilibrium is CaCO3(s) CaO(s) +CO2(g) Given KP =167 bar at 1073 K.
(a.) 1 1.896mol L − (b.) 4 1 4.38 10 mol L − −  (c.) 4 1 6.3 10 mol L −  (d.) 1 6.626 mol L − 14.)At 350 K KP for the reaction given below is 10 1 3.0 10 bar −  at equilibrium. What will be the value of Kc at this temperature? 2N2(g) + O2(g) 2N2O(g) (a.) 11 1 7.4 10 L mol−  (b.) 10 1 8715 10 Lmol−  (c.) 1 0.08Lmol− (d.) 11 1 8.715 10 Lmol−  15.)1 mole of NO and 1 mole of O3 are taken in a 10 L vessel and heated. At equilibrium, 50% of NO (by mass) reacts with O3 according to the equation: NO(g) + O3(g) NO2(g) + O2(g) What will be the equilibrium constant ofr this reaction? (a.) 1 (b.) 2 (c.) 3 (d.) 4 16.)When sulphur is heated at 900 K, S8 si converted to S2 what will be the equilibrium constant for the reaction if initial pressure of 1 atm falls by 25% at equilibrium? (a.) 3 0.75 atm (b.) 3 2.55 atm (c.) 3 25.0atm (d.) 3 1.33atm 17.)For which of the following reactions, KP = Kc ? (a.) PCl3(g) +Cl 2(g) PCl5(g) (b.) H2(g) +Cl 2(g) 2HCl(g) (c.) N2(g) + 3H2(g) 2NH3(g) (d.) CaCO3(s) CaO(s) +CO2(g) 18.)Which of the following relations between the reactions and equilibrium constant for a general reaction, aA + bB cC + dD is not correct? (a.) aA + bB cC + dD : Kc (b.) cC + dD aA + bB: c ' c K 1 K = (c.) naA + nbB ncC + ndD : n c '' Kc = K (d.) aA + bB cC + dD : Kc = KP
19.)In the relation, n P c K K (RT)  = the value of n is (a.) Number or moles of gaseous reactants – number of moles of gaseous products in a balanced equation (b.) Number of moles of gaseous products – number of moles of gaseous reactants in a balanced equation (c.) Number of moles of gaseous products × number of moles of gaseous reactants in a balanced equation (d.) Number of moles of gaseous reactants + number of moles of gaseous products in balanced equation. 20.)For the reaction 2NO2(g) 2 4(g), P Kc N O K / is equal to. (a.) RT 1 (b.) RT (c.) RT (d.) 2 (RT) 21.)5 moles of SO2 and 5 moles of O2 react in a closed vessel. At equilibrium 60% of the SO2 is consumed. The total number of gaseous moles ( SO2, O2 and SO3 ) in the vessel is. (a.) 5.1 (b.) 3.9 (c.) 10.5 (d.) 8.5 22.)In the system X + 2Y Z, the equilibrium concentrations are,       1 1 1 Z 0.216molL X 0.06 mol L , Y 0.12mol L , − − − = = = Find the equilibrium constant of the reaction. (a.) 250 (b.) 500 (c.) 125 (d.) 273 23.)For the reaction N2(g) + O2(g) 2NO , (g) the value of Kc at 800 C o is 0.1. What is the value of KP at this temperature? (a.) 0.5 (b.) 0.01 (c.) 0.05 (d.) 0.1 24.)For the reaction a + b c + d, initially concentrations of a and b are equal and at equilibrium the concentration of d will be twice of that of a. what will be the equilibrium constant for the reaction? (a.) 2 (b.) 9 (c.) 4 (d.) 3 25.)Calculate KP for the equilibrium, NH4HS(s) NH3(g) + H2S(g) If the total pressure inside the reaction vessel is 1.12 atm at 105 C o . (a.) 0.56 (b.) 1.25 (c.) 0.31