Redox reaction is the chemical reaction in which both oxidation (loss of electrons) and reduction (gain of electrons) takes place or transfer of electrons between two species occurs.
The given chemical equation is :
Here, in reactant side, the oxidation state of zinc is zero (0), after reacting with hydrogen chloride, the oxidation sate of zinc becomes two (+2). In this reaction, electrons are transferred from zinc atoms to the hydrogen atoms. Thus, zinc is oxidized by losing electrons.
Hence, oxidation state of zinc increases due to loses electrons i.e. Option (A) is correct.
Coulomb's law mathematically is:
F = kQ₁Q₂/r²
we integrate this with respect to distance to obtain the expression for energy:
E = kQ₁Q₂/r; where k is the Coulomb's constant = 9 x 10⁹; Q are the charges, r is the seperation
Charge on proton = charge on electron = 1.6 x 10⁻¹⁹ C
E = (9 x 10⁹ x 1.6 x 10⁻¹⁹ x 1.6 x 10⁻¹⁹) / (185 x 10⁻¹²)
E = 1.24 x 10⁻¹⁸ Joules per proton/electron pair
Number of pairs in one mole = 6.02 x 10²³
Energy = 6.02 x 10²³ x 1.24 x 10⁻¹⁸
= 746.5 kJ
Answer:
A: Cu; B: Mg; C: Mg + Cu²⁺ ⟶ Mg²⁺ + Cu
Explanation:
The left-hand side of the cell diagram is where oxidation occurs (the anode).
Mg ⟶ Mg²⁺ + 2e⁻
So, Mg is the anode.
The right-hand side of the cell diagram is where reduction occurs (the cathode)
Cu²⁺ + 2e⁻ ⟶ Cu
As the copper ions hit the copper cathode, they remove electrons from the metal and become copper atoms. Since the metal has lost electrons, Cu is the positive electrode.
To get the overall reaction, we add the two half-reactions,
Mg ⟶ Mg²⁺ + 2e⁻
<u>Cu²⁺ + 2e⁻ ⟶ Cu </u>
Mg + Cu²⁺ ⟶ Mg²⁺ + Cu
Try d cuz if im not mistaken if you burnt white phosphorus all the gas is going to take most the air