Consider the equilibrium reaction: Ag2SO4(s) <=> 2Ag+ + SO4-2. What would be the effect of adding more Ag+ in the reaction container?
no effect
equilibrium is reached faster (wrong answer)
equilibrium reaction is shifted forward
equilibrium reaction is shifted in the reverse direction
Ag2SO4(s) <=> 2Ag+ + SO4-2
if we add Ag+
which is a PRODUCT, then the shift will favour
more solid formation, in order to counterbalance the system
so
equilibrium reaction is shifted in the reverse direction
Consider the equilibrium reaction: Ag2SO4(s) <=> 2Ag+ + SO4-2. What would be the effect of adding...
Consider the equilibrium reaction: Ag2SO4(s) <=> 2Ag+ + SO4-2. Which of the following is the correct equilibrium expression for this equation? [Ag+][SO4^-2}/[Ag2SO4] [Ag+]^2 [SO4^-2}/[Ag2SO4] (wrong answer) [Ag+][SO4^-2} [Ag+]^2 [SO4^-2}
When the solution above has reached equilibrium, what effect would adding more Mg2+ have? Adding more F-? Why is it that NO MORE PRODUCT forms when more MgF2 is added to the solution at equilibrium?
6. Answer the following questions regarding the equilibrium for the reaction below 2 AsH3(g) = 2 As (s) + 3 H2 (9) a. If AsH3 was removed from the equilibrium mixture, what would happen to the equilibrium concentration of H2? (increase, decrease, no change) b. If additional As is added to the reaction, what would happen to the equilibrium concentration of AsH3? (increase, decrease, no change) c. If the value of K decreases as the temperature of the system is...
Consider the following reaction. 2Ag^+(aq) + Zn(s) --> 2Ag(s) +Zn(aq) a) write the individual oxidation and reduction half-reactions, specifying which is the anode and which is the cathode reaction. b) calculate the cell potential for a cell containing 0.10M Ag^+ and 0.25M Zn^2+ at 298K. (E ag= 0.80 V and E zn= -0.76 V)
The free energy change for the following reaction at 25 °C, when [Cd2]- 8.59x103 M and [Ag]- 1.17 M, is 244 kJ: Ca2 (8.59x103 M)+ 2Ag(s)Cd(s)+ 2Ag'(1.17 M) AG-244 kJ What is the cell potential for the reaction as written under these conditions? Answer: Would this reaction be spontaneous in the forward or the reverse direction?
The equilibrium constant, Kfor the following reaction is 1.55x0 at 644 When a sufficientiy large sample of HI(g) is introduced into an evacuated vessel at 644 K, the equilibrium concentration of I2)s found to be 0.303 M Calculate the concentration of HI in the equilibrium mixture. more group attempts remaining Submit Anawer Retry Entire Group Consider the following reaction where K 0.159 at 723 K. A reaction mixture was found to contain 2.07x102 moles of N2), 4.45x10-2 moles of H2)...
The free energy change for the following reaction at 25 °C, when [Fe2+1 - 6.16*10' M and (Ag - 1.19 M, is 252 kJ: Fe2+(6.16*109 M) + 2Ag(s) >Fe(s) + 2Ag*(1.19 M) AG = 252 kJ What is the cell potential for the reaction as written under these conditions? Would this reaction be spontaneous in the forward or the reverse direction? We were unable to transcribe this imageThe free energy change for the following reaction at 25 °C, when [Pb2+]...
7 Consider the following reaction at 298 K: NH3(g) +HCI(g)NH4CI(s) Using the thermochemical data at 298 K given below (a) Determine the AH for the reaction. (2 marks) (b) Determine the AG for the reaction and comment on its value. (3 marks) (c) Determine the maximum work done available in the reaction. (3 marks) An equilibrium mixture, consisting of 0.5 atm of NHy(), 0.5 atm of HCKg) and excessive of NH Cl(s), is enclosed in a container at 298 K...
Consider the following reaction where Ke = 1.29x10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) A reaction mixture was found to contain 9.63x10-2 moles of COC1(2), 4.64x10-2 moles of CO(g), and 3.72x10-2 moles of Cl(), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse...
Consider the following reaction where K. = 6.30 at 723 K. 2NH3() N2(g) + 3H2(8) A reaction mixture was found to contain 6.48*10* moles of NH3(g), 2.78 102 moles of N2(e), and 4.23-102 moles of H2(g), in a 1.00 liter container Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the...