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Answer:
0.2 kcal/mol is the value of
for this reaction.
Explanation:
The formula used for is:


where,
= Gibbs free energy for the reaction
= standard Gibbs free energy
R =Universal gas constant
T = temperature
Q = reaction quotient
k = Equilibrium constant
We have :
Reaction quotient of the reaction = Q = 46
Equilibrium constant of reaction = K = 35
Temperature of reaction = T = 25°C = 25 + 273 K = 298 K
R = 1.987 cal/K mol

![=-1.987 cal/K mol\times 298 K\ln [35]+1.987 cal/K mol\times 298K\times \ln [46]](https://tex.z-dn.net/?f=%3D-1.987%20cal%2FK%20mol%5Ctimes%20298%20K%5Cln%20%5B35%5D%2B1.987%20cal%2FK%20mol%5Ctimes%20298K%5Ctimes%20%5Cln%20%5B46%5D)

1 cal = 0.001 kcal
0.2 kcal/mol is the value of
for this reaction.
Answer:
G8 = x0'x2' +x0'x3' +x1x2
Explanation:
The expression can be written different ways, depending on the need to avoid hazards. One of them is ...

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A truth table and Karnaugh map are shown for the circuit. The terms used in the Boolean expression come from the corners, the upper half of the left- and right-columns, and the right half of the middle two rows. If a static hazard is to be avoided, a term x1x0' could be added representing the right column.
Answer:
shoe box covered in aluminum foil