If 1.0 M of A and 3.0 M of B are initially placed into a closed reactor. Which of the following is the value of [A] when the reaction is at equilibrium? 3A(aq) + B(aq) →→2C(aq) + D(aq) O 1.0M 3.0 M OOM O 20M K = 5.5 x 10-5
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Please don't provide handwritten solution .....
![If 1.0 M of A and 3.0 M of B are initially placed into a closed reactor. Which of the following is
the value of [A] when the reaction is at equilibrium?
3A(aq) + B(aq) →→2C(aq) + D(aq)
O 1.0M
3.0 M
OOM
O 20M
K = 5.5 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F666fde10-5362-43c7-843a-0447aaee801d%2Fc2125d6f-a5b1-46b5-93d1-67e39e2b7b1f%2Fede5vqh_processed.jpeg&w=3840&q=75)
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- When 3.0 mole of I2 and 4.0 mole of Br are placed in a 2.0-L rxn chamber at 150 degrees celsius, the following reaction occurs until equilibirum is reached. I2(g) + Br2(g) <--> 2IBr(g) Chemical analysis then shows that the reactor contains 3.2 mole of IBr. What is the equilibrium constant for the reaction ?Reaction CaCO3(s) Ca²+ (aq) + CO3²- (aq) AgCl(s) Ag+ (aq) + Cl(aq) AgBr(s) = Ag*(aq) + Br(aq) Agl(s) Ag+ (aq) + I¯(aq) Initial Concentrations ← [Ca²+] = 1.0 x 10-⁹ M [CO32] = 1.0 x 10⁹ M Ksp = [Ca²+][CO3²-1 X = 3.8 x 10-9 Initial Conditions Q = [1.0 × 10-⁹][1.0 × 10-⁹] = 1.0 x 10-18 Equilibrium Conditions [Ca2+] = 1.0 x 10⁹ M [CO32] 1.0 x 10.⁹ M Mass of CaCO3(s) = 0.0 g 42 of 7 What is the value of the reaction quotient, Q, which is calculated by substituting the actual initial values of [Ca²+] and [CO32] into the equilibrium expression?If 1.0 M of A and 3.0 M of B are initially placed into a closed reactor. Which of the following is the value of [A] when the reaction is at equilibrium? 3A(aq) + B(aq) →→2C(aq) + D(aq) 1.0M O 3.0 M OOM 0 2.0 M K = 5.5 x 10-5
- If 1.0 M of A and 3.0 M of B are initially placed into a closed reactor. Which of the following is the value of [A] when the reaction is at equilibrium? 3A(aq) + B(aq) → 2C(aq) + D(aq) O 1.0M O 3.0 M ООМ 0 2.0 M K = 5.5 x 10-55.00 mol of ammonia are introduced into a 1.00-L reactor vessel in which it partially dissociates at high temperatures according to the reaction. 2NH3(g) <-> 3H2(g) + N2(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. What is Kc for the reaction at this temperature?Consider the reaction. A(aq) = 2 B(aq) Ke 5.32 x 10-6 at 500 K %| If a 5.20 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M %3D
- At 25 °C, Kc = 360. for the reaction AgCl(s) + Br (aq) AgBr(s) + Cl(aq) If solid AgCl is added to a solution containing 0.100 M Br", what will be the equilibrim concentrations of Brand Cl? [CI] = i M eTextbook and Media [Br] = i MIn the reaction, NH3N₂ + H₂, the number of moles of each substance at equilibrium in a 3520mL reactor was found to be NH3 = 0.18 mol, N₂ = 2 mol, and H₂ = 0.23 mol. What is the value of the equilibrium constant?The equilibrium constant for the reaction 6A (aq) + 5B (aq) = 8C (aq) +D (aq) is found to be K = 1.293 * 10-7 %3D What would the equilibrium constant be for the opposite reaction, D (aq) + 8C (aq) = 6A (aq) + 5B (aq) if the concentration for each reactant was increased by a factor of 5? Note: Increasing by a factor of z means multiplying by the factor of z, so A increased by a factor of 2 would be 2A Please express your answer in scientific notation to the third decimal place
- 26 a12) ancl i -2x = 0.76 M = 2 3. Consider the reaction below. What equilibrium pressures of N2, O2, and NO will result when a 10- I reactor vessel is filled with 2.00 atm of N2 and 0.400 atm of 02 and the reaction is allowed to come to equilibrium? L07 N2 (g) + O2 (g) : - 2NO (g); K,= 3.80 x 10 at 2000 °C I 22 04 atm m zatm C -X -X 2x arm atm E 2-x O.4-At T=480.4 °C, when an excess copper (Cu) metal is put into 1.5 M HCl solution, hydrogen gas and CuCl2(s) are expected to be produced in the 10 L reactor. The chemical reaction equation is Cu(:) + 2НС{(аg) — СиCl2(:) + Н2 (9) Please use the following table to calculate the equilibrium partial pressure (bar) of H2 in the reactor at T=480.4 °C. Please write the unit of the pressure in bar! Thermodynamic Data at 25° C. Assume that AH; and S° are independent of temperature. AH:(kJ - mol AG;(kJ - mol-1 Cu(s) HCI (aq) -92.3 -95.27 H2 (g) CuCl2 (s) -220.1 -175.79. The dissolution reactions of gold (Au) in 1M HNO3 and 1M aqua regia (1M HNO3 + 1M HCI) are given below. Au(s) + NO3 + 4 H+, (aq) → Au3+ (аq) + NO(9) + 2 H20(1) (1) (аq) Au(s) + NO3 + 4 H* (aq) (aq) + 4 Cl (aq) → AuCl4" + NO(9) + 2 H200 (2) (аq) (g) Reduction Half – Reaction E° (V) - Au3+ + 3 e- 2 Au 1.36 AuCl4¯ + 3 e¯ → Au + 4 Cl- 1.00 NO3- + 4 H* + 3 e¯ → NO + 2 H20 0.96 2 H30* + 2 e-= H2 + 2 H20 9. a) Calculate E°cell and Keg for the dissolution of gold in 1M HNO3 under standard conditions. 9. b) Calculate E°cell and Keg for the dissolution of gold in aqua regia under standard conditions. 9. c) Using the values calculated in a) and b), determine the formation constant (K;) of AuCla". The formation reaction is given below. [Hint, express Kf as a function of the Keg values from a) and b)]. 3+ Aušt (aa) + 4 Cl¯ (ад) → AuCl4 (aq)
