Given the followingstandard enthalopy , values: A: +15.7KJmol^ -1 : B: - 86.4 * k / (mo * l ^ (- 1)) ; C: - 52.7kjmo *...
1)For the process Ao → Ag) , the AHwR = 30.5 kJ/mol and ASm"-86.4 J/molK. Assuming these values are independent of T, what is the normal boiling point of substance A in °C? Do not input the unit just numerical value (the number). 2) For a certain process at 355 K, ΔG =-12.4 kJ and ΔH--72 kJ. What is the change in entropy,AS, for this process? 3)Consider the following hypothetical reaction (at 310 K). Standard free energies. AGP, in kJ/mol...
เต Use the References to access important values if needed for this question. Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(g)--C4H10(g) ΔΗ。=-125.6 kJ (2) C2H4(8) 2C(s)+ 2H2 AH -52.3 k what is the standard enthalpy change for the reaction: (3) 2C2H4(g) + H2(g)--C41110(g) ΔΗ·"? 1 pr pr 1 pt 1 pt 1 pt 1 pt Submit Answer Try Another Version 2 item attempts remaining
References Use the References to access important values if needed for this question. Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(g)—1C4H10(g) AH° = -125.6 kJ (2) C2H2(g) →2C(s) + 2H2(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C2H4(E) + H2(9) >C_H10(8) AH° = ? Submit Answer
Use the References to access important values if need Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(9) C4H10(9) AH° = -125.6 kJ (2) C2H4(9)— 2C(s) + 2H2(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C2H4(g) + H2(g)—>C4H109) AH° = ? Submit Answer Retry Entire Group 2 more group attempts remaining
Use the data given here to calculate the values of AG xn at 25 °C for the reaction described by the equation Compound А 4G (kJ/mol) +387.7 +590.4 B A+B=0 с +402.0 AG KJ I AHin and ASi. are both negative values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is enthalpy-driven to the right O enthalpy-driven to the left. st & 0 $ 8 9 B A+B= +590.4 +402.0 с AGX =...
Use the data given here to calculate the values of AGxn at 25 °C for the reaction described by the equation Compound A AG, (kJ/mol) +387.7 A+B C B +514.5 с +402.0 AGRX = kJ If A Hixn and ASin are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is enthalpy-driven to the right entropy-driven to the left. enthalpy-driven to the left. O entropy-driven to the right.
Use the data given here to calculate the values of delta G^degree _rxn at 25^degree C for the reaction described by the equation A + B double headed arrow C If delta D^degree _rxn and delta S^degree _rxn are both negative values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is entropy-driven to the right. entropy-driven to the left. enthalpy-driven to the left. enthalpy-driven to the right.
Hess's Law 6. Given the following data: C(graphite) C(diamond); AH -+1.897 k Coo(fullerene); AHo+2193 k) 60 C(graphite) calculate the standard enthalpy of reaction for the conversion of buckminsterfullerene (Co) Into diamond: 1/60 Ceo (fullerene) C (diamond) 7. Given the following thermochemical data at 25°C and 1 atm pressure: O2(g) +2 B(s) B2O3(s), AHo-1264 k) O3(9) +2 B(s) calculate the standard enthalpy for the following reaction: B2O3(s), AHo=-1406 k) 2 O3(g) 3 O2(g) b
Suppose the firm's production function is given by f(K,L) = min {K",L"} (a) For what values of a will the firm exhibit decreasing returns to scale? Constant returns to scale? Increasing returns to scale? (b) Derive the long-run cost function and the optimal input choices. (c) Suppose the capital is fixed at K = 10,000 and a = 1. Assuming that the firm wants to produce less than 100 units, derive
Use the data given here to calculate the values of AGfxn at 25 °C for the reaction described by the equation Compound AG; (kJ/mol) +387.7 -623.9 В A B C +402.0 С AGxn = kJ If AHixn and ASPxn are both negative values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is O enthalpy-driven to the left. entropy-driven to the left. O enthalpy-driven to the right O entropy-driven to the right