9) For a particular reaction ??--32 kJ and AS-.98 JK. a. At what temp will the...
For a particular reaction, ΔH = -32 kJ and ΔS =-98 J/K. Assume that ΔH and ΔS do not vary withtemperature. A) At what temperature will the reaction have ΔG= 0? B) If T is increased from that in part A, will the reaction bespontaneous or nonspontaneous?
For the reaction CO2(g) + H2(9)—-CO(g) +H30(9) AH° = 41.2 kJ and A Sº = 42.1 JK The equilibrium constant for this reaction at 252.0 K is Assume that AH and AS are independent of temperature. For the reaction N2(g) + 3H2(g) 2NH3(g) AH° = -92.2 kJ and AS™ = -198.7 J/K The equilibrium constant for this reaction at 347.0 K is Assume that AHⓇ and AS are independent of temperature.
at a temperature is 8.314 JK 2 For a given reaction, with AH = -19.9 kJ/mol and AS = -55.5 J K mol at a 12. Calculate the equilibrium constant. The Universal gas constant is 82 (25 points)
The activation energy of a particular reaction is 83.1 kJ/mol. By what factor will the rate constant increase when the temperature is increased from 50 °C to 60 °C?
A reaction has an enthalpy change of - 71 kJ mol" and an entropy change of -58 JK-mol-. At what temperature does this exothermic reaction cease to be spontaneous? 422°C 673°c 826°C O 951°C What is the molar reaction enthalpy for the reaction below: N2H4(0) +CHNO(0) 4CHẠO(g) +Ng(g) + 3H (g) given the following thermodynamic data? 2NH3(9) ► N2H4(l) + H2(9) A,Hm = 22.5 kJ mol-1 2NH3(9) N2(g) + 3H2(9) A Hm = 57.5 kJ mol-1 CH,0(9) + H2(g) +...
QUESTION 7 A particular reaction has a ΔΗο value of-186 kJ and ΔGo of-118 kJ at 599 K. Calculate ASO at 599 K in JK 0
QUESTION 9 A particular reaction has a DH ° value of -172 kJ and DS of 42 J/K at 298 K. Calculate DG at 407 K in kJ (with 3 significant digits), assuming that DH and S hardly change with temperature
For the reaction 2HBr(g) + Cl2(g)—>2HCl(g) + Brz(9) AH° = -81.1 kJ and AS° = -1.2 J/K The equilibrium constant for this reaction at 269.0 K is Assume that AHⓇ and AS are independent of temperature. Submit Answer Retry Entire Group 8 more group attempts remaining For the reaction N2(g) + 3H2(g) +2NH3(g) AH° = -92.2 kJ and A Sº = -198.7 JK The equilibrium constant for this reaction at 308.0 K is Assume that AHⓇ and AS are independent...
For the reaction, PCI5 (g) <> PCI3 (g) + CI (g) DELTA H = 398.KJ MOL-1 the equilibrium constant, K , was calculated to be 11.5 at 600 K what will happen to the value of the equilibrium constant if the temperature is increased? A) decrease B) increase C) remain the same D) cannot be determined from the information provided
Question 13 For the reaction with AH = 30 kJ/mol at equilibrium 2NOBrig = 2ND which of the following will happen if the temperature is increased K does not change. K will decrease More NOBr will be produced NO will be consumed MK will increase