How to solve this problem step by step
1 answer:
Answer:
Explanation:
Hello there!
In this case, according to the given information, it turns out possible for us to solve this problem by using the combined gas law:
Thus, we solve for the final volume by solving for V2 as follows:
Now, we plug in the variables to obtain the result in milliliters and making sure we have both temperatures in Kelvins:
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Answer: The standard cell potential (E∘) for the reaction is -0.121 V
Explanation:
The reaction is:
Relation between standard Gibbs free energy and equilibrium constant follows:
where,
= Standard Gibbs free energy = ?
R = Gas constant =
T = temperature = 298 K
K= equilibrium constant =
Putting values in above equation, we get:
To calculate standard Gibbs free energy, we use the equation:
Where,
n = number of electrons transferred = 1
F = Faradays constant = 96500 C
= standard cell potential = ?
Putting values in above equation, we get:
Thus standard cell potential (E∘) for the reaction is -0.121 V