kiki197701

01.04.2020 • 

Chemistry

Given the following standard reduction potentials at 25°C:
Half reaction
Ag (aq) + e → Ag (S)
Cu(ag) + 2e → Cu (S)
Ni?' (ag) + 2e → Ni (s)
Cr+ (aq) + 3e → Cr(s)
Reduction Potential (V)
+ 0.80
+0.34
- 0.28
-0.74
1. Combine these reduction half-reactions into a redox reaction (hint-one will be a
reduction, the other will be an oxidation) such that the Ecell is the smallest positive value
possible.
Balanced redox reaction:
Eceh
mV
2. What is 'n' from the reaction above? n=
moles electrons
3. What is delta G and is this reaction spontaneous or not? delta G=
4. What is K?K=
5. Is the reaction product-favored or reactant favored?

Ответ:

chhimmidemg

20.04.2023

Chemistry

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 3.36 L of ammonia gas

Explanation:

The balanced chemical reaction is:

 

According to stoichiometry :

3 moles of produce = 2 moles of

Thus 0.75 moles of will producee=  of

But as percent yield is 30 %, amount of ammonia produced =

According to ideal gas equation:

P = pressure  = 1 atm

V = Volume  = ?

n = number of moles = 0.15

R = gas constant =

T =temperature =

Thus 3.36 L of ammonia gas is obtained by reacting 0.75 moles of hydrogen with excess nitrogen.

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