Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron-transfer reaction.
Fe2+(aq) + Ag+(aq) ---> Fe3+(aq) + Ag(s)
| species oxidized | species reduced | |
|---|---|---|
| oxidizing agent | reducing agent | |
| As the reaction proceeds, electrons are transferred from | to | . |
3Fe3+(aq) + Al(s) ---> 3Fe2+(aq) + Al3+(aq)
| species oxidized | species reduced | |
|---|---|---|
| oxidizing agent | reducing agent | |
| As the reaction proceeds, electrons are transferred from | to |
. |
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron-transfer reaction.
2Cr2+(aq) + Hg2+(aq) --->2Cr3+(aq) + Hg(s)| species oxidized | species reduced | |
|---|---|---|
| oxidizing agent | reducing agent | |
| As the reaction proceeds, electrons are transferred from | to | . |
When NO(g) reacts with O2(g) to form NO2(g), 13.6 kcal of energy are evolved for each mole of NO(g) that reacts.
Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank.
| + | + | + |
When HCl(g) reacts with O2(g) to form H2O(g) and Cl2(g), 6.84 kcal of energy are evolved for each mole of HCl(g) that reacts.
Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank.
| + | + | + | + |
When Fe3O4(s) reacts with H2(g) to form Fe(s) and H2O(g) , 36.1 kcal of energy are absorbed for each mole of Fe3O4(s) that reacts.
Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank.
| + | + | + | + |
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