Balance the following redox reaction if it occurs in h2so4. what are the coefficients in front of c3h8o2 and h2so4 in the balanced reaction? c3h8o2(aq) + k2cr2o7(aq) → c3h4o4(aq) + cr2(so4)3(aq)

3C3H8O2 and 16H2SO4

Explanation:

C3H8O2(aq) + K2Cr2O7(aq) → C3H4O4(aq) + Cr2(SO4)3(aq)

In acidic reaction you need to separate the half-reactions knows.

C3H8O2(aq)  → C3H4O4(aq)

Cr2O7(2-) → Cr(+3) (aq)

Balance elements other than O and H. Add H2O to balance oxygen, balance hydrogen by adding protons (H+) and Balance the charge of each equation with electrons

C3H8O2(aq) + 2H2O(l)  → C3H4O4(aq) + 8H(+) + 8e(-)

Cr2O7(2-) + 14H(+) + 6e(-) → 2Cr(+3) + 7H2O (aq)

Scale the reactions so that the electrons are equal. If not look for a common multiple. In this case is 24, 8*3=6*4. So for each equation multiply for the correct multiple. Then

3C3H8O2(aq) + 6H2O(l)  → 3C3H4O4(aq) + 24H(+) + 24e(-)

4Cr2O7(2-) + 56H(+) + 24e(-) → 8Cr(+3) + 28H2O (aq)

Add the reactions and cancel out common terms and group the ions in compounds if u can.

3C3H8O2(aq)  + 32H(+) + 4Cr2O7(2-)  → 3C3H4O4(aq) + 4Cr2(SO4)3(aq) + 22H2O (aq)

We are in acidic medium  so the H(+) must be from H2SO4. So 32H(+) is  16H2SO4 in reactives. Add SO4(2-) in products and balance

16H2SO4 +3C3H8O2(aq) + 4Cr2O7(2-)  → 3C3H4O4(aq) 4Cr2(SO4)3(aq) + 22H2O (aq) + 4SO4(2-)

Then

16H2SO4 +3C3H8O2(aq) + 4Cr2O7(2-)  → 3C3H4O4(aq) 4Cr2(SO4)3(aq) + 22H2O (aq) +  + 2K2SO4 (aq)

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.