For the conversion of ice to water at 0°C and 1 atm, ΔG is zero, ΔH is positive, and ΔS is positive. ΔG is zero, ΔH is positive, and ΔS is negative. ΔG is negative, ΔH is positive, and ΔS is negative. ΔG is positive, ΔH is zero, and ΔS is positive.
For the conversion of ice to water at 0°C and 1 atm, ΔG is zero, ΔH...
The sign of ΔG will be negative when ΔS is positive and ΔH is positive ΔS is negative and ΔH is positive ΔS is positive and ΔH is negtive ΔS is negative and ΔH is negative
The conversion of solid CO2 ("dry ice") to CO2 gas is product-favored at room temperature. What would be the signs for ΔG, ΔH, and ΔS at room temperature? CO2(s) --> CO2(g) ΔG = (+) ΔH = (+) ΔS = (-) ΔG = (-) ΔH = (+) ΔS = (-) ΔG = (+) ΔH = (+) ΔS = (+) ΔG = (-) ΔH = (+) ΔS = (+) ΔG = (-) ΔH = (-) ΔS = (+)
For the sublimation of CO2 at 0 C and 1 atm: a) ΔS<0, ΔG<0 b) ΔS>0, ΔG<0 c) ΔS>0, ΔG>0 d) ΔS<0, ΔG>0 e) ΔS>0, ΔG=0
(3) Find ΔS for the conversion of 18.0g of ice at 0 ° C and 1.00 atm to 18.0g of water vapor at 100 ° C and 2.00atm. ΔHf = 33.6 J/g ΔHf = 2256.7 J/g Cp = 4.19 J/gK
A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) PCl3(g) + Cl2(g) → PCl5(g) ΔHf° (kJ mol-1) -287.0 -374.9...
2. For a process where ΔH⁰sys < 0 and ΔS⁰sys> 0, when is the sign on ΔG⁰sys < 0? a. ΔG⁰sys is never less than zero b. ΔG⁰sys < 0 for all temperatures c. ΔG⁰sys < 0 for low temperatures d. ΔG⁰sys < 0 for high temperatures 3. For a process where ΔH⁰sys < 0 and ΔS⁰sys< 0, when is the sign on ΔG⁰sys < 0? a. ΔG⁰sys < 0 for high temperatures b. ΔG⁰sys < 0 for all temperatures...
A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) 3 PbO2(s) → Pb3O4(s) + O2(g) ΔHf° (kJ mol-1) -277.0...
Calculate ΔS and ΔG for the evaporation of 1 mol water at T = 100°C and p = 1 atm. The latent heat of evaporation of water is 9.7 kcal/mol.
At equilibrium, the free energy change, ΔG, of any system is zero: ΔG=0=ΔH−TΔS So, under equilibrium conditions, this equation can be rearranged as T=ΔHΔS Part A Glacial acetic acid is the concentrated form of acetic acid, the acid in vinegar. The term "glacial" refers to the appearance of the solid form, which resembles glacial ice. What is the melting point of this compound, in degrees Celsius, based on its thermodynamic data shown here? ΔHfus (kJ/mol) = 24.32 ΔSfus [J/(K⋅mol)] =...
For the freezing of liquid hexane, C 6H , at a given temperature and pressure, ΔH is negative and ΔS is negative. ΔH is positive and ΔS is positive. ΔH is negative and ΔS is positive. ΔH is positive and ΔS is negative.