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disa [49]
3 years ago
9

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second c

olumn will increase the entropy S of the system, decrease S, or leave S unchanged. If you don’t have enough information to decide, check the “not enough information “button in the last column.

Chemistry
1 answer:
kiruha [24]3 years ago
4 0

Answer:

For each system listed in the first column of the table below, decide (If possible) whether the change described in the second column will Increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the not enough information" button in the last column.

System As A few grams of water vapor (H,0). The water condenses to a liquid at a not enough The carbon dioxide is heated from -5.0 °C to 13.0°c and is also compressed from a volume of 9.0 1 to a volume of 5.0L A few moles of carbon dioxide (CO2) gas. not enough information -15.0 °C to 86.0 °C while the volume is held constant at 2.0 L A few moles of carbon dioxide (CO,) gas. S > 0 not enough 1 Don't Know

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The equilibrium constant is given as :

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K_p=K_c\times (RT)^{\Delta n}

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Now put all the given values in the above relation, we get:

K_p=14.45\times (0.0821L.atm/K.mol\times 293.15 K)^{-2}

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