Which occurs in the half-reaction Na(s) → Na+ + e−? *

A. Na(s) is reduced
B. Na(s) is oxidized
C. Na(s) gains electrons
D. Na+ is oxidized

A. Na(s) is reduced

Explanation:

In order for reduction to occur, the atom must gain an electron. And in this reaction, the Na(s) went from a 0 to +1

**Remember: Lose Electrons = Oxidized and Gain Electrons = Reduced

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !