Calculate the change in entropy of the surroundings when 54.0 g of methanol boils at 64.7°C. The heat of vaporization for CH3OH is 35.278 kJ/mol.
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Calculate the change in entropy of the surroundings when 54.0 g of methanol boils at 64.7°C....
The heat of vaporization of CH_2CI_2 is 28.0 kJ/mol. Calculate the entropy the entropy change when 42 g of CH_2CI_2 boils at its boiling point of 39.8degreeC. 17 J/K 44J/K 59J/K 350J/K 700J/K
Sample problems 3: How does the entropy of the system change when the following occur: a) a so vaporizes; ce) a solid dissolves in water; d) a gas liquefies? as 2. The normal boiling point of methanol (CHsOH) is 64.7 Co, and its molar enthalpy of vaporization is Hap -71.8 kJ/mol. A) When CHoOH 1) boils at its normal boiling point, does its entropy increase or decrease? B) Calculate the value of AS when 1.00 mol of CHOH() is vaporized...
The heat of vaporization AH, of ethyl aceae4Hs 35.1 kJ/mol. Calculate the change in entropy AS when 4.6 g of ethyl acetate boils at Be sure your answer contains a unit symbol. Round your answer to 2 significant digits
This question asks: Calculate the change in entropy that occurs in the system when 1.00 mol of methanol (CH3OH) vaporizes from a liquid to a gas at its boiling point (64.6 degrees Celcius). For methanol, enthalpy of vaporization = 35.21 kJ/mol I'm getting the correct answer (104) but I'm getting a negative for some reason, and the book says it's positive, but the formula changeinEntropy = -enthalpy of system/T, so why isn't this number negative?
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