Which of the following is an oxidation-reduction reaction? group of answer choices h2co3 (aq) + ca(no3)2 (aq) → 2hno3 (aq) + caco3 (s) agno3 (aq) + hcl (aq) → agcl (s) + hno3 (aq) ba(c2h3o2)2 (aq) + na2so4 (aq) → baso4 (s) + 2nac2h3o2(aq) cu (s) + 2agno3 (aq) → 2ag (s) + cu(no3)2 (aq) hcl (aq) + naoh (aq) → h2o (l) + nacl (aq)

Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq) is an oxidation -reduction reaction

Explanation:

An oxidation-reduction reaction is a chemical reaction that involves a transfer of electrons between two atoms, molecles,.. It is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron.

⇒The oxidation state of an individual atom is 0.

⇒The total oxidation state of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge.

⇒Group 1 metals have an oxidation state of +1 and Group 2 an oxidation state of +2

⇒Hydrogen generally has an oxidation state of +1 in compounds

⇒Oxygen generally has an oxidation state of -2 in compounds

H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s)

Carbon on the left has an oxidation state of -4, on the right it has also oxidation state -4

Nitrogen has on the left an oxidation state of +5, on the right it has also an oxidation state of +5

Calcium has on the left an oxidation state of +2, on the right also an oxidation state of +2

⇒ There is no change of oxidation number so this is NOT a redox reaction

AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO3

Silver (Ag) on the left has an oxidation state of +1, on the right it has also oxidation state +1

Nitrogen has on the left an oxidation state of +5, on the right it has also an oxidation state of +5

Cl has on the left an oxidation state of -1, on the right it has also an oxidation state of -1

⇒ There is no change of oxidation number so this is NOT a redox reaction

Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2(aq)

Na has on the left an oxidation state of +1, on the right it has also an oxidation state of +1

Ba has on the left an oxidation state of +2, on the right it has also an oxidation state of +2

S has on the left an oxidation state of +6, on the right it has also an oxidation state of +6

⇒ There is no change of oxidation number so this is NOT a redox reaction

Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq)

Cu has on the left an oxidation state of 0, on the right it has an oxidation state of +2

Ag has on the left an oxidation state of +1, on the right it has also an oxidation state of 0

⇒ There is a change of oxidation number so this is a redox reaction

Oxidizing agent: Ag in AgNO3 ; Reducing agent: Cu

HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq)

Na has on the left an oxidation state of +1, on the right it has also an oxidation state of +1

Cl has on the left an oxidation state of -1, on the right it has also an oxidation state of -1

Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq) is an oxidation -reduction reaction

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.