The student plotted the experimental kinetics data  as ln[A] versus time and obtained a straight line graph for the hypothetical reaction aA =>bB.  If k is a rate constant, then the slope of the line must equal to:

Use the Nernst equation to calculate the cell potential for the following cell in Volts: Cr|Cr3+, 0.0010M||Cu2+, 1.0M|Cu To receive full credit (2 pts for answer and 2 pts for showing work), submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL

Many electronic calculators use rechargeable nickel–cadmium batteries. The overall equation for the spontaneous reaction in these cells is: Cd(s) +NiO2(s) + H2O(l) → Cd(OH)2(s) + Ni(OH)2(s) What are the oxidation states of Cd in Cd and of Ni in NiO2 and Ni(OH)2? 

The presence of a catalyst:

How does a salt bridge keep the reaction going?

Balance the chemical equation given below, and determine the number of milliliters of 0.105 M phosphoric acid required to neutralize 35.00 mL of 0.0550 M calcium hydroxide.   ________ Ca(OH)2(aq) + ________ H3PO4(aq) → ________ Ca3(PO4)2(s) + ________ H2O(l) To receive full credit (2 pts for answer and 2 pts for showing work), submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL

What is an equivalence point in titration strong base with the strong acid?

On the illustration of a generic cell for In/Zn electrodes immersed in their salt solutions 1. Use numbers from the picture to identify (5 pts) :  the anode:  the cathode: the direction of cations  the direction of anions the direction of the electrons flow 2.   In3++3e−⟶In     Eo= −0.3382V Zn2++2e−⟶Zn    Eo= −0.7618V Use the given electrode potentials above to write the following (10 pts): the anode half-reaction (2 pts) the cathode half-reaction (2 pts) the balanced overall net equation the cell voltage produced (4 pts) the standard cell notation (2 pts) Calculate Eocell(5 pts) To receive credit, report your answers below and submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL ANSWERS:  

Which of the following is a balanced molecular equation describing the titration of a strong acid with a strong base? 

The graph below shows the titration of the aqueous solution containing 0.148 g of unknown monoprotic acid solution with 0.101M NaOH. Assignment and rubric: Use the proper graphing techniques to answer the questions about an unknown acid (24pts). You may print the graph from the exam or download it from the Exam Module. Showing calculations and answers is required for credit. The picture of your work on the graph is NOT required although it may be helpful for PC. equivalence point:          VNaOH ; pH (4pts) half-equivalence point: VNaOH; pH (4pts)                                             pKa;    Ka; (4+4=8 pts);                                            molar mass (MM), (8 pts).          To receive credit, report your answers below and submit a picture of your work to the Final Exam Required Work & Partial Credit  assignment AFTER SUBMITTING COMPLETED FINAL ANSWERS: