Concept explainers
Practice ProblemBUILD
Like equilibrium constants. values are temperature dependent. At
The corresponding cell reaction is:
Calculate the equilibrium constant for this reaction at
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- What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is 6.55x10-3 atm, the H* concentration is 1.00M, and the Al3+ concentration is 8.73x10-4M? 6H*(aq) + 2Al(s)3H₂(g) + 2Al³+ (aq) Answer: The cell reaction as written above is spontaneous for the concentrations given:.arrow_forwardWhat is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H2 pressure is 7.53×10-3bar, the H+ concentration is 1.15 M, and the Zn2+ concentration is 5.73×10-4 M ? 2H+(aq) + Zn(s) H2(g) + Zn2+(aq)Answer: VThe cell reaction as written above is product-favored (spontaneous) for the concentrations givenarrow_forwardThe reaction Ni+Cl2→Ni^(+2)+2Cl^- has an overall cell potential equivalent to 1.59 V. Is the reaction spontaneous? *full explanation pleasearrow_forward
- hat is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 3.68×10-4 M and the Mg2+ concentration is 1.25 M ?Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq)Answer: ___The cell reaction as written above is spontaneous for the concentrations given: true or false?arrow_forward5.Calculate ΔG° for the following balanced redox reaction. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) given the following standard redox potentials: Pb2+(aq) + 2e- ⟶⟶ Pb(s) E0 = -0.13 V Cu2+(aq) + 2e-⟶⟶ Cu(s) E0 = 0.34 V Group of answer choices -41 kJ -047 kJ +46 kJ +91 kJ -21 kJarrow_forwardConsider a cell reaction at 25°C where n=4 . Fill in the following table.arrow_forward
- Consider a cell reaction at 25°C where n=2 . Fill in the following table.arrow_forwardConsider a cell reaction at 25oC where n=3. Fill in the following table.∆Go Eo Ka. 24kJ ? ?b. ? 0.120V ?c. ? ? 0.114arrow_forwardWhat is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H2 pressure is 1.33×10-3 bar, the H+ concentration is 1.31 M, and the Al3+ concentration is 4.95×10-4 M ?6H+(aq) + 2Al(s)------>3H2(g) + 2Al3+(aq) Answer: ____Varrow_forward
- Calculate Ecell at 25.0 oC using the following half-reactions with [Fe+2] = 1.00 M, [Fe+3] = 0.00100 M, [Cl-1] = 0.00300 M and PCl2 = 0.500 atm. Fe+3(aq) + 1e-1 →Fe+2(aq) Cl2(g) + 2e-1 →2Cl-1(aq) Group of answer choices 1.841 V 2.417 V 0.300 V 1.250 V 0.712 V 0.875 Varrow_forwardWhat is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H2 pressure is 1.08×10-3 atm, the H+concentration is 1.30M, and the Co2+ concentration is 9.41×10-4M ? 2H+(aq) + Co(s) ---->H2(g)+ Co2+(aq)Answer: ______VThe cell reaction as written above is spontaneous for the concentrations given: _______t or f.arrow_forwardZn + Ag+ Zn2+ + Aga) Write the cell according to the accepted notation for a voltaic cell, including the polarity ofthe electrodes, phase boundaries, salt bridge.b) Write the anode, cathode and total reactions, balance the reaction and calculate the totalcell potential.c) If the enthalpy of the reaction at 25°C is, ΔH°298 = 51820 cal/mol, find the values of ΔG°298and ΔS°298.d) Decide whether the reaction is spontaneous or not at standart conditions.e) If Zn metal is immersed in the solution containing Ag+ions and it is electrolyzed byapplying 1 A for 3 hours, how many grams of Ag are coated?E°Zn2+/Zn = -0.763 V, E°Ag+/Ag = 0.80 V, MAg = 107 g/molarrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning