Answer:
A catalyst is a substance that can be added to a reaction to increase the reaction rate without getting consumed in the process. Catalysts typically speed up a reaction by reducing the activation energy or changing the reaction mechanism.
Explanation:
Answer:
using three significant figures, to match the data
v = 51.4
p = -0.999
In an endothermic reaction products are <u>HIGHER </u>than reactants in potential energy and <u>LESS </u>stable.
Explanation:
Energy is input into the reaction in an endothermic reaction. This means the products are of a higher energy level than the reactants. Therefore the reaction increases Gibb's free energy and reduces entropy. Remember in thermodynamic stability involves an increase in entropy and a decrease in Gibbs free energy. Therefore the products are less stable than the reactants. This is why endothermic reactions do not occur spontaneously like exothermic reactions.
Answer: from the lies this is synthesis reaction
Explanation:
It's also oxidation-reduction reaction. Li is oxidised and
H is reduced
where, E^{o} (Ag+/Ag) = std. reduction potential of Ag+ = 0.7994 v
and Sn2+/Sn = std. reduction potential of Sn2+ = -0.14 v
Thus, E^{o}cell = 0.7994v - (-0.14v) = 0.9394 v
Now, ΔG^{o} = -nF
,
where, n = number of electrons = 2
F = Faraday's constant = 96500 C
∴ΔG^{o} = 2 X 96500 X 0.9394 = -1.18 X
Now, using Nernst's Equation we have,
![[tex]E_{cell} = 0.9394 - \frac{2.303X298}{2X96500}log \frac{0.0115}{ 3.5^{2} }](https://tex.z-dn.net/?f=%20%5Btex%5DE_%7Bcell%7D%20%3D%200.9394%20-%20%5Cfrac%7B2.303X298%7D%7B2X96500%7Dlog%20%5Cfrac%7B0.0115%7D%7B%203.5%5E%7B2%7D%20%7D%20)
E_{cell} = 0.9765 v
Finally, ΔG = -nFE = -2 X 96500 X 0.9765 = -1.88 X
