Question

Choose the reaction that involves reduction/oxidation.

1) c(s) + o2(g) ��� CO������(g)
2) h(aq) + oh-(aq) ��� h2o(l)
3) ba2(aq) + (SO���)���-(aq) ��� baso4(s)
4) 2 naf + cacl2 ��� 2 nacl + caf2

Answer 1

The reaction that involves reduction/oxidation is the combustion of carbon to form carbon dioxide (C + O2 → CO2), as it involves a change in oxidation states.

Step-by-step explanation:

To identify which of the given reactions involves a reduction/oxidation process, also known as a redox reaction, we need to look for changes in oxidation states of elements in the chemical reactions provided.

1. C(s) + O2(g) → CO2(g) - In this reaction, carbon (C) is oxidized as it goes from an oxidation state of 0 to +4 (for the C in CO2); oxygen (O2) is reduced as it goes from 0 to -2 in CO2. This is a redox reaction.
2. H(aq) + OH-(aq) → H2O(l) - This is an acid-base neutralization reaction; there are no changes in oxidation states.
3. Ba2+(aq) + SO4^2-(aq) → BaSO4(s) - This is a precipitation reaction where a solid forms from two aqueous ions; there is no change in oxidation states.
4. 2 NaF + CaCl2 → 2 NaCl + CaF2 - This is a double displacement reaction where ions exchange partners, with no change in oxidation states observed.

Therefore, the reaction involving reduction/oxidation is the combustion of carbon to form carbon dioxide (C + O2 → CO2).