Consider the following reaction of calcium hydride (cah2) with molten sodium metal: cah2(s) 2 na(l) -> 2 nah(s) ca(l) identify the species being oxidized and the species being reduced.

None of the species in the equation have undergone either oxidation or reduction

Explanation:

The easiest way to see if oxidation or reduction has happened is to compare oxidation numbers of each and every species before and after the reaction.

Calcium is two before the reaction and two after the reaction

Hydrogen is -1 before the reaction and -1 after the reaction

Sodium is one before the reaction and one after the reaction

Iodine is -1 before the reaction and -1 after the reaction.

For an oxidation to happen an increase in oxidation number has to happen.

For a reduction to happen, a decrease in oxidation number has to happen. None have happened

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: