Using the virtual lab (link above), create a nickel concentration cell where one cell is 2 M and the other is 0.0001 M. What is the \Delta\text{G}_{\text{cell}} Δ G cell of the cell? Report your answer in kJ.
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Using the virtual lab (link above), create a nickel concentration cell where one cell is 2...
Using the virtual lab (link above), create a nickel concentration cell where one cell is 2 M and the other is 0.0001 M. What is the \Delta\text{G}_{\text{cell}} Δ G cell of the cell? Report your answer in kJ.
Using the virtual lab (link above), create a zinc concentration cell where one cell is 1.53 M and the other is 0.0084 M. What is the EMF of the cell? Note: Record the value for the spontaneous reaction.
Question 4 2 pts Using the virtual lab above and Appendix C in your lab manual, complete the following statement Note: Record the values for the spontaneous reaction. A Ag/Ni voltaic cell has an Eo of V. If you change the concentration of the solution in each cell to 0.01 M, the EMF is V. This change is because the standard potential, Eo is defined at M, so K, atm, and differing from those standard conditions will change the observed...
An electrochemical cell is constructed such that on one side a pure nickel electrode is in contact with a solution containing Ni2+ ions at a concentration of 5*10-3 M. The other cell half consists of a pure Fe electrode that is immersed in a solution of Fe2+ ions having a concentration of 0.3 M. At what temperature will the potential between the two electrodes be +0.140 V?
A copper-nickel (35 wt % - 65 wt %) alloy is corroded in an oxygen-concentration cell using boiling water. What volume of oxygen gas (at 1 atm) must be consumed at the cathode to corrode 54 g of the alloy? (Assume only divalent ions are produced.) Express your answer to three significant figures.
Consider a uniport system where a carrier protein transports an uncharged substance A across a cell membrane. Suppose that at a certain ratio of [A]_inside to [A]_outside, the delta G for the transport of substance A from outside the cell to the inside, A_outside rightarrow A_inside, is 11.1 kJ/mol at 25 degree C. What is the ratio of the concentration of substance A inside the cell to the concentration outside? [A]_inside/[A]_outside = Choose the true statement about the transport of...
A galvanic cell is assembled from one half cell with a nickel electrode immersed in Ni 2+ aqueous solutions in one beaker where [Ni2+] = 1.2 M coupled to a second half cell with a chromium electrode immersed in a Cr3+ aqueous solution to give Ecell = +0.55 V at 25 °C. 3Ni2+(aq) + 2Cr(s) → 3Ni(s) + 2Cr3+(aq) Eϴ cell = +0.50 V Calculate the concentration of the chromium ions [Cr3+] in solution. (A) 1.9 x10^–1 M (B) 6.7...
Determining pH using a Concentration Cell
Part A - Determining pH Using a Concentration Cell A concentration cell constructed from two hydrogen electrodes, both with PH2 = 1.00. One electrode is immersed in pure H2O and the other in 6.0 M hydrochloric acid. What is the emf generated by the cell and what is the identity of the electrode that is immersed in hydrochloric acid?
Consider a galvanic cell where one compartment has Br2 (aq) at a concentration of 0.50 M and Br ̄ at a concentration of 0.10 M with a platinum electrode and the second compartment has Cr3+ at a concentration of 0.20 M and a Cr electrode. Use the following reduction potentials to answer the questions: Cr3+ (aq) + e ̄→Cr(s) εo = - 0.73 V Br2(aq) + 2e ̄→2Br ̄ (aq) εo =1.09V a. What is the standard cell potential for...
A Zn/Zn2+ concentration cell has a voltage of 0.204 V at 25 ∘C. The concentration of Zn2+ in one of the half-cells is 1.49×10−3 M . What is the concentration of Zn2+ in the other half-cell? (Assume the concentration in the unknown cell to be the lower of the two concentrations.) Express your answer using 2 decimal places and in pM. (p = pico = 10-12)