0
What else can I help you with?
What is the standard reduction potential E for the half reaction Mg2 aq 2e Mgs?
-2.37 V (apex) Chace
What is the overall voltage for a redox reaction with the half reactions Mg s -- Mg2 plus plus 2e- and Cu2 plus -- Cu s?
The standard reduction potentials for Mg/Mg^2+ and Cu^2+/Cu are -2.37 V and +0.34 V, respectively. To determine the overall cell potential, you subtract the reduction potential of the anode (Mg/Mg^2+) from the reduction potential of the cathode (Cu^2+/Cu) since the anode is where oxidation occurs. Therefore, the overall cell potential would be 0.34 V - (-2.37 V) = 2.71 V.
What is the overall voltage for a redox reaction with the half-reaction Mg s Mg2 2e- and Cu2 2e- Cu s?
0.34 - (-2.37) you're welcome.
What is the cation for MgCl2?
The cation for MgCl2 is Mg2+.
What are the half reactions for a galvanic cell with Zn and Mg electrodes apex?
Zn2+(aq) +2e- => Zn(s) and Mg(s) => Mg2+(aq) + 2e-
What is the standard reduction potential E for the half reaction Mg2 aq 2e Mgs?
-2.37 V (apex) Chace
What is the standard reduction potential e for the half-reaction mg2 (aq) 2e?
-2.37 v
What is the standard reduction potential E for the half-reaction Mg2 (aq) 2e Mg(s)?
-2.37 v
What is the standard reduction potential E for the half-reaction Mg2 (aq) 2e- Mg(s)?
-2.37 v
What is the overall voltage for a redox reaction with the half reactions Mg s -- Mg2 plus plus 2e- and Cu2 plus -- Cu s?
The standard reduction potentials for Mg/Mg^2+ and Cu^2+/Cu are -2.37 V and +0.34 V, respectively. To determine the overall cell potential, you subtract the reduction potential of the anode (Mg/Mg^2+) from the reduction potential of the cathode (Cu^2+/Cu) since the anode is where oxidation occurs. Therefore, the overall cell potential would be 0.34 V - (-2.37 V) = 2.71 V.
What is the overall voltage for a redox reaction with the half-reaction Mg s Mg2 2e- and Cu2 2e- Cu s?
0.34 - (-2.37) you're welcome.
If you have Mg and after a reaction you then have Mg2 what happened to cause this change?
Mgnesium lost two electrons (reduction).
What is the reduction half-reaction for Mg(s) ZnCl2(aq) MgCl2(aq) Zn(s)?
Mg(s) Mg2+ + 2e-
Calculate the standard emf of a cell that uses the Mg Mg2 plus and Cu Cu2 plus half cell reactions at 25 degrees C?
Cu + Mg2 --------> Cu2 + Mg Cu --------------> Cu2 + 2e Mg2 + 2e --------> Mg Cu --------------> Cu2 + 2e (E = +0.35) Mg2 + 2e --------> Mg (E = -2.36V) +0.35 + (-2.36) = -2.01V --------------------------------------… Mg + Cu2 --------> Mg2 + Cu Mg --------------> Mg2 + 2e Cu2 + 2e --------> Cu Mg --------------> Mg2 + 2e (E = +2.36V) Cu2 + 2e --------> Mg (E = -0.35V) +2.36 + (-0.35) = +2.01V
Do magnesium and copper sulphate react?
No. This is a redox question. It is asking whether the reaction will occur spontaneously. In order for Mg+2 to spontaneously oxidize Cu(s), Mg+2 needs to have a higher reduction potential (the tendency to be reduced) than Cu+2. Check a redox table to see: Mg2+ + 2 e− --> Mg(s) E° = −2.372 Cu2+ + 2 e− --> Cu(s) E° = +0.340 (More favorable reaction) Cu2+ has a higher reduction potential, meaning Mg2+ will not oxidize Cu(s).
What is the oxidation half reaction of mgs plus zncl2aq mgcl2aq plus zns?
It is the zinc that gets reduced, and the magnesium that gets oxidised. This is because zinc has the higher reduction potential of -0,76 V, compared to magnesiums -2,37 V. The oxidation half cell therefore becomes Mg (s) --> Mg2++ 2e-
What is the cation for MgCl2?
The cation for MgCl2 is Mg2+.
