
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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What is the equilibrium constant K at 25 °C for an
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- Given the balanced electrochemical reaction below (M and N represent generic metals), what is the cell potential (Ecell), in volts, for this reaction at 35.4 °C when [M+] = 0.00533 M and [N2+] = 0.725 M? Enter your answer to the thousandths place. Do not include units. 2M+(aq) + N(s) → 2M(s) + N2+(aq) E°cell = 0.128 Varrow_forwardWhat is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0165 V and n = 2?(F = 96,500 J/(V・mol), R = 8.314 J/(mol・K))arrow_forwardIf an alkaline battery produces a cell potential of 1.66 V, what is the value (in kj) of ΔGcell? The half-reactions in alkaline batteries are: ZnO(s) + H2O(l) + 2e^- --------> Zn(s) + 2OH^- (aq) 2MnO2(s) + H2O(l) + 2e^- -----------> Mn2O3(s) + 2OH^- (aq)arrow_forward
- A certain metal M forms a soluble nitrate salt M(NO3). Suppose the left half cell of a galvanic cell apparatus is filled with a 4.00 M solution of M(NO3), and the right half cell with a 200. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left ☐ x10 rightarrow_forwardA certain metal M forms a soluble sulfate salt M, SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 250. mM solution of M,SO, and the right half cell with a 2.50 M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. left Which electrode will be positive? Ox10 right ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.arrow_forwardThe standard cell potential (E°cell) of the reaction below is -0.55 V. The value of A G° for the reaction is J/mol. 12 (s) + 2Br" (aq) → 21 (aq) + Br2 (1) 0.55 5.5 · 5. 10-6 1.1· 105 0.54 none of the abovearrow_forward
- Calculate the cell voltage at 25°C for this cell when [H+] = [HSO4–] = 4.5 M. At 25°C, E° = 2.04 V for the lead-acid battery. For this reaction, ∆H° = –315.9 kJ and ∆S° = 263.5 J/mole K. Calculate E° at –20° C and Ecell when [H+] = [HSO4–] = 4.5 M.arrow_forwardWhat is the equilibrium constant K at 25°C for an electrochemical cell when E° = %3D +0.0290 V andn= 2?(F = 96,500 J/(V· %D mol), R = 8.314 J/(mol·K)) %3D tvarrow_forwardWhat is the maximum amount of work that is possible for an electrochemical cell where E = 1.58 V and n = 2? (F = 96,500 J/(V・mol))arrow_forward
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