Using the relative e0 values determine which of the following reactions are electrically possible. mg(s) + br2(i) ⟶ mgbr2 choose the answer from the parenthesis. this equation shows that mg is (reduced or oxidized) this equation shows that br2 is (reduced or oxidized) can this redox reaction take place? (yes or no)

To determine if the reaction provided is electrically possible, we can first separate the overall reaction into its half-reactions:

Mg (s) + Br₂ (l) → MgBr₂ 

Mg → Mg²⁺ + 2e⁻           E = -2.37 V

Br₂ + 2e⁻ → 2Br⁻            E = 1.09 V

Looking at the half-reactions, we can see that magnesium loses electrons in the process which means that magnesium is oxidized.

Since bromine is gaining electrons, Br₂ is being reduced.

Now to determine if this reaction is taking place, we must find the reduction potentials for each half-reaction. To final the overall potential of the cell, we take the difference in the cathode (reduction) and anode (oxidation) potentials.

Ecell = Ecathode - Eanode

Ecell = 1.09 V - (-2.37 V)

Ecell = 3.46 V

A positive value of Ecell means that the reaction will happen spontaneously. Therefore, this reaction is electrically possible and will take place.

the catch is that the top numbers are atomic masses the bottom numbers are the numbers of protons and electrons in an uncharged atom. they are the number of that atoms as you would find them on the periodic table. further, the numbers on the left are used to determine the missing numbers on the right

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer