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1.0 M acid and two pt electrodes connected to a voltmeter. You then add 10.00 ml of 1.00 M Fe^+2 solution to the beaker. The temperature of the solution is maintained at 25 C.(R= 8.314 coulomb V/(mol K), F= 9.64853 x 10^4 coulomb/mol)
A) Write the standard half-cell reduction reaction equation for reactive species in the beaker.
B) Determine the cell potential(Ecell) at the moment of mixing.
C) Determine the equilibrium constant(Keq) for the reaction system.
D) if enough of the 1.00 M Fe^+2 solution is added to reach the equivalence point, determine the new cell potential.
E) Determine the cell potential(Ecell) if 20.0 ml of 1.00 M Fe^+2 solution is added to the solution.
write the rate law for each elementary reaction in the mechanism. D) if the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction.
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Consider 4.00 rm L of a gas at 365 rm mmHg and 20. rm ^{circ}C . If the container is compressed to 3.00 rm L and the temperature is increased to 36, rm ^{circ}C, what is the new pressure, P_2, inside the container? Assume no change in the amount o..
Calculate the percent enantiomeric excess of the contents of the bottle labeled as just menthol. For the purchased sample what percentage of (-)-menthol is indicated by this measurement?
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