At what temperature is this reaction spontaneous?
2H2(g)+O2(g)⟶2H2O(g)ΔH∘=−241.82kJ;ΔS∘=−88.75J/K
At what temperature is this reaction spontaneous? 2H2(g)+O2(g)⟶2H2O(g)ΔH∘=−241.82kJ;ΔS∘=−88.75J/K
Consider the reaction 2H2O(g) →2H2(g) + O2(g) ΔH = +483.60 kJ/mol at a certain temperature. If the increase in volume is 27.7 L against an external pressure of 1.00 atm, calculate ΔU for this reaction. (The conversion factor is 1 L· atm = 101.3 J.) _______kJ
Consider the reaction 2H2O(g) → 2H2(g) + O2(g) ΔH = +483.60 kJ/mol at a certain temperature. If the increase in volume is 42.7 L against an external pressure of 1.00 atm, calculate ΔU for this reaction. (The conversion factor is 1 L · atm = 101.3 J.) _______kJ
ΔS is negative for the reaction ________. 2H2O (g) → 2H2 (g) + O2 (g) LiOH (aq) → Li+ (aq) + OH– (aq) CH3OH (l) → CH3OH (g) Sr(NO3)2 (aq) + 2LiOH (aq) → Sr(OH)2 (s) + 2LiNO3 (aq) C6H12O6 (s) → 6C (s) + 6H2 (g) + 3O2 (g)
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
If ΔH = -70.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature.
The elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O,H2O, H2,H2, and O2O2 reach 0.0200 atm,0.0200 atm, 0.00550 atm,0.00550 atm, and 0.00700 atm,0.00700 atm, respectively. What is the value of the equilibrium constant at this temperature? kp= ?
If ΔH = -70.0 kJ and ΔS = -0.300 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.
If ΔH = -80.0 kJ and ΔS = -0.500 kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature Express your answer numerically in kelvins.
For the reaction ΔH°=+61.14 kJ and ΔS° = +132 J/K at 25°C. At what For the reaction ΔH°=+61.14 kJ and ΔS° = +132 J/K at 25°C. At what minimum temperature will the reaction be spontaneous?minimum temperature will the reaction be spontaneous? Select one: a. 479 K b. 500 K c. 463 K d. 571 K e. 2904 K
Hydrogen gas reacts with oxygen to form water. 2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 233 kJkJ of heat.