5. Consider the reaction of carbon monoxide with oxygen to produce carbon dioxid

Question

5. Consider the reaction of carbon monoxide with oxygen to produce carbon dioxide. 2 CO(g) + Oz(g) 2 CO2(g) At what temperature will this reaction be spontaneous according to Gibb's Energy? AH in kJ/mol for: CO()-110.5, CO.(g) -393.5 AS in J/mol K for: CO(g) - 197.6, CO.(g) - 213.6, O(g) 205.0 ics, the us a. temps above-63.1 K 4 b. temps below 179.5 K c. temps above 415.8 K d. temps below 3273 K 6. The randomness of a system may be described as its: C a. Gibb's energy C b. entropy C c. kinetic energy C d. enthalpy 7. Two 6.5 L flasks are joined by a 150 mL tube with a stop cock. If 0.25 moles of nitrogen are held in the left flask and the right flask is empty, what happens to the entropy of the system upon opening the valve between the flasks? ( g) = a. The entropy remains the same. b. The entropy decreases c. There is too little information to assess the change. d. The entropy increases. 8. Without detailed calculations, predict the sign of AS for the system for:

Explanation / Answer

the answer of 6th question id option d

it can explain as firtd to calcolate H by the formula i.e (total enthaply of product)*no of moles of product- no. of moles of reactant(total enthalpy of reactant)

now calculate S bysame as above. now H=-566kj/mol and S =-17 J/mol K now since we need G negative for spontaneous process so the equation become G=H-TS shoul de less than zero i.e.

H-TS<0 and substituting the value we get T<3273K.

ANSWER OF QUESTION 6 is b its entropy which decide the randomness

answer of question 7 is the entropy of system increases as the area now increases where nitrogen gas is

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