Chemistry, 30.08.2019 03:30 jay9253

For a galvanic cell that uses the following two half-reactions, cr 2o 7 2-( aq) 14 h ( aq) 6 e - → 2 cr 3 ( aq) 7 h 2o( l)sn( s) → sn 2 ( aq) 2 e -how many moles of sn(s) are oxidized by four moles of cr 2o 7 2-

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Answer from: broyochey1

Answer : The number of moles of Sn(s) oxidized are 12 moles.

Explanation :

The given half cell reactions are:

Reduction half reaction : $Cr_2O_7^{2-}(aq)+14H^+(aq)+6e^-\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

Oxidation half reaction : $Sn(s)\rightarrow Sn^{2+}(aq)+2e^-$

In order to balance the electrons, we will multiply oxidation half reaction by 3, we get:

Reduction half reaction : $Cr_2O_7^{2-}(aq)+14H^+(aq)+6e^-\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

Oxidation half reaction : $3Sn(s)\rightarrow 3Sn^{2+}(aq)+6e^-$

Now adding both half reaction, we get the overall reaction.

$Cr_2O_7^{2-}(aq)+14H^+(aq)+3Sn(s)\rightarrow 2Cr^{3+}(aq)+3Sn^{2+}(aq)+7H_2O(l)$

From the overall complete reaction, we conclude that

As, 1 mole of $Cr_2O_7^{2-}$ will oxidizes 3 moles of Sn

So, 4 moles of $Cr_2O_7^{2-}$ will oxidizes $4\times 3=12$ moles of Sn

Therefore, the number of moles of Sn(s) oxidized are 12 moles.

Answer from: Quest

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .

Answer from: Quest

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:

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For a galvanic cell that uses the following two half-reactions, cr 2o 7 2-( aq) 14 h ( aq) 6 e - → 2...

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