Given the unbalanced equation, enter the formula and state of the product that f

Question

Given the unbalanced equation, enter the formula and state of the product that formed as a result of the oxidation of its precursor (oxidation product). If more than one answer exists, separate by a comma.

Ba(s) + H2O(l) ? Ba2+(aq) + OH-(aq) + H2(g)

Given the unbalanced equation, for the species that accepts electrons, enter the symbol and the initial oxidation state of the specific element that will go to a lower oxidation state.

Enter sign followed by Arabic numeral for oxidation state magnitude. Use 0 if the oxidation state is zero.

Example:

Element: S

Oxidation state: -2

Given the balanced equation, enter the formula and state of the reduction product that formed from the oxidizing agent. If more than one answer exists, separate by a comma.

Sn(s) + 2Ag+(aq) + 2ClO4-(aq) ? 2Ag(s) + Sn2+(aq) + 2ClO4-(aq)

Given the balanced equation, indicate whether Li+(aq) formed as a direct result of reduction (R), oxidation (O), both (B) or neither (N). You may enter the abbreviation without parenthesis.

2Li(s) + 2H2O(l) ? 2Li+(aq) + 2OH-(aq) + H2(g)

Given the unbalanced equation, enter the formula and state of the species that is reduced. If more than one answer exists, separate by a comma.

Sn(s) + HBr(aq) ? SnBr2(aq) + H2(g)

Given the balanced equation, for the species that forms from the oxidizing agent, enter the symbol and the final oxidation state of the specific element that was reduced. Use arabic numerals for oxidation state magnitude.

Example:

Element: Sb

Oxidation state: 0

Explanation / Answer

1. Ba, Oxidation State : +2 (Ba is oxidized to Ba(+2))

2. H, Oxidation State : +1 (H(+1) accepts electron to form H in reduced form)

3. Ag, Oxidation State : 0 (Ag(+1) is getting reduced to form Ag)

4. Oxidation (Li is being oxidized to Li(+1))

5. H, Oxidation State: +1 (H(+1) is being reduced to H)

6. H, Oxidation State : 0 (H(+1) is being reduced to H)

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