Chemistry, 06.04.2021 03:30 dwighthibbert56
Consider the electrochemical constructed using the spontaneous cell reaction, Ni(NO3)2(aq) + Zn(s) = Zn(NO3)2(aq) + Ni(s)
The diagram devoid this cell with the two metal electrodes - cathode on the right - and two aqueous solutions. The salt bridge is filled with potassium nitrate.
Which of the following statements are true regarding this electrochemical cell? (You can choose as many)
a) Electrons flow in the wire from anode to cathode
b) The solution on the left is Ni(NO3)2(aq)
c) Nickel ions are reduced at the cathode
d) The cathode is Ni(s)
e) Zinc ions are reduced at the anode
f) The anode is Ni(s)
Answers: 2
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The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)
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Consider the electrochemical constructed using the spontaneous cell reaction, Ni(NO3)2(aq) + Zn(s) =...
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