For the following reaction CCl4 (g) → C(s) + 2 Cl2 (g) Ho = +95.7 KJ;...
For the following reaction CCl4 (g) → C(s) + 2 Cl2 (g) Ho = +95.7 KJ; So = +142.2 J/K 1) What is Go for this reaction at 25 C? 2) What is the equilibrium constant for this reaction at 100 C? I need help with number 2) why would you not recalculate delta G for the reaction because its at a different temperature than 25C?
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For the following reaction CCl4 (g) → C(s) + 2 Cl2 (g)
Ho = +95.7 KJ;...
The reaction CCl4--> C(graphite) + 2Cl2 has delta H= +95.7 kJ and delta S= +142.2 J/K...
The reaction CCl4--> C(graphite) + 2Cl2 has delta H= +95.7 kJ and delta S= +142.2 J/K at 25 degrees C. Calculate delta G.
Consider the reaction: 2Cl2(g) + SO2(g) -> SOCl2(g) + Cl2O(g) Cl2(g) SO2(g) SOCl2(g) Cl2O(g) (delta)Hof (kJ/mol):...
Consider the reaction: 2Cl2(g) + SO2(g) -> SOCl2(g) + Cl2O(g) Cl2(g) SO2(g) SOCl2(g) Cl2O(g) (delta)Hof (kJ/mol): 0 -296.8 -212.5 80.3 So (J/K*mol): 223.1 248.1 309.77 266.2 (delta)Gof (kJ/mol): 0 -300.13 -198.3 97.9 A) Use the given data to calculate (delta)Go for the reaction and state specifically if the reaction is product or reactant favored at equilibrium. B) At what temperature will (delta)Go change sign?
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations:...
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations: C(s)+H2(g)-->CH4 H= -74.6 kJ C(s) + Cl2(g)--> CCl4 H=-95.7 kJ H2(g)+Cl2(g)--> HCl H=-92.3 kJ
11) a) For the reaction H2(g) + Cl2(g) ---> 2 HCl(g) G° = -190.8 kJ and...
11) a) For the reaction H2(g) + Cl2(g) ---> 2 HCl(g) G° = -190.8 kJ and S° = 20.0 J/K at 309 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 309 K. The standard enthalpy change for the reaction of 2.34 moles of H2(g) at this temperature would be ___ kJ. b) For the reaction CO(g) + Cl2(g) ---> COCl2(g) H° = -108 kJ and S° = -137 J/K G° would be negative at temperatures...
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta...
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta S° = -128.9 J/K The equilibrium constant for this reaction at 306.0 K is _______? Assume that Delta H° and DeltaS° are independent of temperature. B) For the reaction N2(g) + 3H2(g)---->2NH3(g) Delta H° = -92.2 kJ and Delta S° = -198.7 J/K The equilibrium constant for this reaction at 333.0 K is ___? Assume that Delta H° and Delta S° are independent of...
Calculate ΔHrxn for the following reaction: CH4 (g) + 4Cl2(g) → CCl4(g) + 4HCl(g) Using the...
Calculate ΔHrxn for the following reaction: CH4 (g) + 4Cl2(g) → CCl4(g) + 4HCl(g) Using the following reactions: C(s) + 2H2(g) → CH4(g) ∆H = -74.6 kJ C(s) + 2Cl2(g) → CCl4(g) ∆H = -95.7 kJ H2(g) + Cl2(g) → 2HCl(g) ∆H = -184.6 kJ
CCl4(g) <---> C(s) + 2 Cl2 (g) , Kp=0.86 If 2.50 atm of CCL4 is added...
CCl4(g) <---> C(s) + 2 Cl2 (g) , Kp=0.86 If 2.50 atm of CCL4 is added to a flask and allowed to reach equilibrium. What are the final pressures of CCl4 and Cl2 at equilbrium?
Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6...
Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6 kJΔH=−95.7 kJΔH=−184.6 kJ
For the reaction 2HBr(g) + Cl2(g)—>2HCl(g) + Brz(9) AH° = -81.1 kJ and AS° = -1.2...
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: H2S(g) + 2H2O(l)3H2(g) + SO2(g) H° = 295 kJ and S° = 295...
For the reaction: H2S(g) + 2H2O(l)3H2(g) + SO2(g) H° = 295 kJ and S° = 295 J/K The equilibrium constant, K, would be greater than 1 at temperatures Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that delta H° and delta S° are constant. For the reaction Fe2O3(s) + 2Al(s)Al2O3(s) + 2Fe(s) H° = -852 kJ and S° = -37.0 J/K The equilibrium constant, K, would be greater than 1...
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...
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