Given that cu + 2hci cu2+ + 2ci- + h2(g) has an overall reduction potential of –0.34 v, what is a valid prediction about how this reaction works? the reaction is not spontaneous and will require energy to proceed. the reverse reaction would require energy input in order to occur. the half reactions would both occur spontaneously. the reaction is not spontaneous, and it is impossible to make it occur.

  Cu + 2HCI → Cu²⁺ + 2CI⁻ + H2(g)

has an overall reduction potential of –0.34 V      

The correct option is:

The reaction is not spontaneous and will require energy to proceed.

Since  the overall reduction potential is negative,the reaction is not spontaneous and it requires energy to proceed.

The reaction is

Cu(s) + 2HCI(aq)  ---> Cu⁺² + 2CI⁻ + H₂(g)

The given E⁰cell = -0.34

The overall reduction potential is negative

A reaction is said to be spontaneous it is ΔG° is negative

The relation between ΔG° and Electrode potential is

ΔG° = -nFE°cell

as given that

E°cell = -0.34 V

The overall value of ΔG° will be positive and hence reaction must be non spontaneous

so

The reaction is not spontaneous and will require energy to proceed.

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.