Question
In: Chemistry
10. The initial and final entropy of a system are 42.9 J/mole*K and 267.2 J/mole*K, respectively....
10. The initial and final entropy of a system are 42.9 J/mole*K and 267.2 J/mole*K, respectively. At a temperature of 86.3oC, the enthalpy associated with this process was +68.6 KJ/mole.
(a) Calculate the number of configurations that the system can assume finally.
(b) Calculate the change of entropy for the system, in J/mole*K. Also, state whether the system became more or less disorderly.
(c) Calculate the Gibb’s free energy for the process, in KJ/mole
(d) State whether the process above is spontaneous, non-spontaneous, or already at equilibrium.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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A very nice (an interesting) formula for the entropy of a system is S=−k∑=1p(ni) lnp(ni), where...
A very nice (an interesting) formula for the entropy of a system
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Consider the standard free energies shown below(T =37 C, R=8.3145 J/mole K) : UDP-Mannose + H2O...
Consider the standard free energies shown below(T =37 C,
R=8.3145 J/mole K) :
UDP-Mannose + H2O → Mannose 1-phosphate + UMP + 2H+ delta G' =
-34.9 kJ/mol
UTP + H2O → UMP + PPi + 2H+ delta G' = -32.5 kJ/mol
PPi + H2O → 2Pi delta G' = -33.6 kJ/mol
(A) ( 2 pts) Calculate delta G' & Keq’ for the following
reaction.
Mannose 1-phosphate + UTP + H2O → UDP-mannose + 2Pi
(B) ( 2 pts) Which...
Consider the standard free energies shown below(T =37 C, R=8.3145 J/mole K) : UDP-Mannose + H2O...
Consider the standard free energies shown below(T =37 C,
R=8.3145 J/mole K) :
UDP-Mannose + H2O → Mannose 1-phosphate + UMP + 2H+ delta G' =
-34.9 kJ/mol
UTP + H2O → UMP + PPi + 2H+ delta G' = -32.5 kJ/mol
PPi + H2O → 2Pi delta G' = -33.6 kJ/mol
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reaction.
Mannose 1-phosphate + UTP + H2O → UDP-mannose + 2Pi
(B) ( 2 pts) Which...
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a. what is the probability of drawing a flush ( all 5 cards are
the same suit)?
b. What is the probability of drawing a full house ( 3 cards of
one value, 2 cards of a different value)?
(Use combinational probability)...
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