Use the thermodynamic data provided below to estimate the
boiling point (in K) of CCl4. Report your answer to zero
decimal places in standard notation (i.e. 123. kJ *For numbers
ending in zero, be sure to include the decimal!*).
Substance | ΔH°f (kJ/mol) | S° (J mol-1K-1) | ||
CCl4 (l) | -128.4 | 214.4 | ||
CCl4 (g) | -96 | 309.6 |
Use the thermodynamic data provided below to estimate the boiling point (in K) of CCl4. Report...
Use the thermodynamic data provided below to estimate the boiling point (in K) of V. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) V (l) 17.3 36.1 V (g) 515.5 182.3
Use the vapour pressures (at 25 °C) of the pure substances below to answer the following questions р* (КРa) Substance 3-methyl-1-butanol (C5H120) 0.315 ethyl formate (C3H602) 32.3 1. Determine the partial pressure (in kPa) of ethyl formate (C3H602) in the vapour phase (at 25 °C) over a solution for which the mole fraction of 3-methyl-1-butanol (C5H120) is 0.322. Report your answer to three significant figures in scientific notation. Tries 0/13 Submit Answer 2. A solution of 3-methyl-1-butanol (C5H120) and ethyl...
no
book?
3. Determine the standard melting point of CCl4 using the following thermodynamic data: Substance AH S®(J/mol K) CCl4 (g) CCl4 (1) -106.7 -193.3 309.4 214.4
3. Determine the standard melting point of CCl4 using the following thermodynamic data: Substance AH S°(J/mol K CCl4 (g) CCl4 (1) -106.7 -193.3 309.4 214.4
3. Determine the standard melting point of CCl4 using the following thermodynamic data: Substance AH S°(J/mol K) CCl4 (9) CC14 (1) -106.7 -193.3 309.4 214.4
Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). C2H2(g) + Br2(g) → C2H2Br2(g)
Using the data provided in the Table, calculate the various entropies below for H2S(aq) ⟶ H+(aq) + HS-(aq) Enter your numbers to 1 decimal places. substance or Ion ΔH°f (kJ/mol) S° (J/mol K) H2S(aq) -39 122 H+(aq) 0 0 HS-(aq) -17.7 61.1 Calculate ΔSsystem (J/K) Calculate ΔSsurrouding (J/K) Calculate ΔSuniv (J/K)
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)> Fe20,(s) ДН/ (kJ/mol) So (J/K-mol) FeO(s) -271.9 60.75 Fe(s) Fe203 (a) 618.1°C 27.15 205.0 89.96 0 -822.16 (b) 756.3°C (c) 1235°O (d) 2439°C (e) spontaneous at all temperatures
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)>...
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 185.98 kJ/mol ΔS∘rxn 27.40 J/(mol⋅K) Calculate the temperature in Kelvin above which this reaction is spontaneous. Express your answer to 0 decimal places and in K.
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 179.97 kJ/mol ΔS∘rxn 22.99 J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 295.9 K: Whatever answer you get multiply by 1x1031 and enter that number to 4 decimal places.