Calculate ΔS∘rxn for the following balanced chemical equation: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g)
Substance and state S∘[J/(K⋅mol)]
H2O(g) 188.8
O2(g) 205
H2S(g) 205.7
SO2(g) 248.1
Calculate ΔS∘rxn for the following balanced chemical equation: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance and stat...
Calculate ΔS∘rxn for the balanced chemical equation H2S(g)+2O2(g)→H2O(g)+SO3(g) Express the entropy change to four significant figures and include the appropriate units. Standard enthalpies for selected substances at 25∘C Substance S∘(J/(mol⋅K)) O2(g) 205.2 SO2(g) 248.2 SO3(g) 256.8 H2O(g) 188.8 H2S(g) 205.8
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
Determine ΔG◦rxn using the following information. 2H2S(g)+3O2(g) ---> 2H2O(l)+2SO2(g) ΔH= +1.12kJ ;ΔS= -390.7J/K
Determine delta G(not) rxn using the following information. Assume standard cognitions. 2H2S(g) +3O2(g) --> 2H2O(l)+2SO2(g) Delta H (not): 1.12 kJ Delta S(not): -390.7 J/K
Consider the following balanced chemical equation: 2H2S(g) + SO2(g) → 3S(s) + 2H2O(g) a. How many moles of H2S must react to form 4.18 moles of S? _ moles H2S b. How many moles of SO2 must react to form 4.18 moles of S? _ moles SO2 c. How many moles of H2S must react to form 4.18 moles of H2O? _ moles H2S d. How many moles of SO2 must react to form 4.18 moles of H2O? _ moles...
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
Calculate the standard-state entropy for the following reaction: 2NiS(s) + 3O2(g) -> 2SO2(g) + 2NiO(s) The standard entropy values are given in the table. Formula S - J/K SO2(g) 248 NiO(s) 38.0 NiS(s) 53.0 O2(g) 205
For the reaction: 2H2S(g) + 3O2(g)2H2O(g) + 2SO2(g) deltaH = -1.04×103 kJ and S° = -153 J/K The equilibrium constant, K, would be greater than 1 at temperatures (above, below) _____ Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.
For the reaction 2 H2S(g) + 3O2(g) ---> 2H2O(g) + 2SO2(g), the initial rate of consumption for O2 is 0.0471 M/s for the first 46 seconds. What is the concentration of H2O after 46.0 seconds?
Calculate ΔG° (kJ/mole) at 298 K for the reaction below:2H2S(g) + 3O2(g) ⇋2H2O(g) + 2SO2(g)K=6.32×1010Enter a number to 2 decimal places.