For H2SO4, Ka,1 is very large and pK2 = 1.96 at 25 °C. For 0.00105 molLH2SO4(aq) at 25 °C, calculate: (a) the equilibrium concentration of the singly-ionized form, HSO4 [HSO, Jeq = Number mol L-1 (Enter a number accurate to 2 significant figures.) (b) the fraction, a2, of H2SO4 that exists in the doubly-ionized form, SO,2- a2= Number (Enter a number between 0 and 1, accurate to 2 significant figures.) (c) the pH pH = Number %3D (Enter a number accurate to 2 decimal places.)

For H2SO4, Ka,1 is very large and pK2 = 1.96 at 25 °C. For 0.00105 molLH2SO4(aq) at 25 °C, calculate: (a) the equilibrium concentration of the singly-ionized form, HSO4 [HSO, Jeq = Number mol L-1 (Enter a number accurate to 2 significant figures.) (b) the fraction, a2, of H2SO4 that exists in the doubly-ionized form, SO,2- a2= Number (Enter a number between 0 and 1, accurate to 2 significant figures.) (c) the pH pH = Number %3D (Enter a number accurate to 2 decimal places.)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

2) 2.44 mol of gaseous hydrogen bromide is added to an empty 3.16 L container. When values are no longer changing, at 62.5 °C, 0.55 mol hydrogen gas is collected. Using the provided skeletal equation, determine the value of the equilibrium constant, at 62.5 °C, to 2 decimal Br2(8) HBr f Bre) Brie) + H, 2(8) [K5] places:
At 800 K, the equilibrium constant for the reactionA2(g)⇌ 2 A(g) is Kc = 3.1 x 10-4. (a) Assuming bothforward and reverse reactions are elementary reactions,which rate constant do you expect to be larger, kf or kr?(b) If the value of kf = 0.27 s-1, what is the value of krat 800 K? (c) Based on the nature of the reaction, do youexpect the forward reaction to be endothermic or exothermic?(d) If the temperature is raised to 1000 K, willthe reverse rate constant kr increase or decrease? Will thechange in kr be larger or smaller than the change in kf ?
Hydrogen gas and bromine gas are mixed in a sealed container at 250°C and allowed to reach equilibrium. H2(g) + Br2(g) = 2HB1(g) The equilibrium constant for this reaction at 250°C is 65.5. At equilibrium, the concentration of H2 is 0.0510 mol L*1 and the concentration of Brris 0.174 mol L-1 at 250°C. (i) Write the equilibrium constant expression for the above reaction. (ii) Calculate the concentration of HBr in the equilibrium mixture at 250°C (iii) Explain what happens to the concentration of HBr you calculated in (ii) above if the pressure of the equilibrium mixture is increased.
The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) +You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, andthe concentration of NH3 is 0.85 M.(a) Calculate the value of the reaction quotient Q.(b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed toreach equilibrium.
Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). (a) O,(g) 503(s K. = 8.70 × 10-9 |× 10 K. = (Enter your answer in scientific notation.) (b) 30,(g) 5 203(g)
Write the equilibrium-constant expression for the reaction A(s) + 3 B(1) ⇒ 2 C(aq) + D(aq) in terms of [A], [B], [C], and [D], as needed. Note that Kc, which is sometimes symbolized as Keq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, Kc means the same thing as Keq. Kc =
Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + Cl2(g)= 2NOCI(g) is 7 x 10° at a certain temperature. In an experiment, 6.70 × 102 mole of NO, 1.00 × 103 mole of Cl2, and 6.80 moles of NOCI are mixed in a 2.10–L flask. What is Qc for the experiment? x 10 (Enter your answer in scientific notation.) In which direction will the system proceed to reach equilibrium? The reaction will proceed to the left. The reaction is at equilibrium. The reaction will proceed to the right.
Use the data in the supporting materials to calculate the equilibrium constant (Kp) for the following reaction at 25°C. 2 SO2(g) + O2(g) =2 S03(g) Кра 4.24e24 Calculate Kp for the reaction at 49°C using the following equations. (a) the van't Hoff equation below. (P), A,H° RT? a In K Кр = 1.138e22 (b) the Gibbs-Helmholtz equations below to find A-G° at 49°C and hence, Kp at the same temperature. AG ΔΗ (i) = - T2 A-G2 A;G1 1 (ii) T2 T1 T1 Kp = 1.138e22 (c) A-G° = ArH° – TA¡S° to find A-G° at 49°C and hence, Kp at the same temperature. Кр 3D 1.7742е22 State the approximations employed in each case. The assumption that A,H° is temperature independent and equal to the value calculated at 298.15 K is required by all three parts A second assumption that AS° is temperature independent and equal to the value calculated at 298.15 K is required by part (c) Compare your results. The answers calculated in parts (a) and (b) ▼ in part (c) are very close as expected because the formulas used to…
Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). 2 (a) O2(g) S,03(g) K = 8.58 × 10-9 %3D х 10 (Enter your answer in scientific notation.) (b) 302(g) 5 203(g)
Use the References to access important values if needed for this question. The equilibrium constant in terms of pressures for the reaction C,H;CH,OH(g)=C,H;CHO(g) + H2(g) is K, = 0.558 at 523 K. (a) A pure sample of gaseous benzyl alcohol, C,H¿CH,OH(g), is introduced into a rigid flask at a temperature of 523 K so that its original pressure is 0.132 atm. Calculate the fraction of this starting material that is converted to products at equilibrium. (b) A second sample of benzyl alcohol is introduced into a rigid flask at a temperature of 523 K, this time at an original pressure of 4.14 atm. Again, calculate the fraction of the starting material that is converted to products at equilibrium.
Write the equilibrium constant expression, K, for the following reaction: If either the numerator or denominator is blank, please enter 1 Ag2SO3(s) =2Ag+(aq) + SO3²-(aq) K =- %3D
The equilibrium constant for the synthesis of ammonia N2(g) + 3 H2(g) --> 2 NH3(g) has the value K = 3.19 × 10^-4 at 400°C. Calculate the equilibrium partial pressures of N2(g), H2(g), and NH3(g) if the total pressure is 1.00 atm and the H:N atomratio in the system is 3;1. (Hint: Try the approximationthat PN2 and PH2 > PNH3 and see if the resulting equationsare simpliied.)