Find ΔHrxn for the following reaction:
2PbS(s)+3O2(g)→2PbO(s)+2SO2(g)
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Find ΔHrxn for the following reaction: 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g)
A) 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g), ΔH∘=−844 kJ, ΔS∘=−165 J/K Express the Gibbs free energy in kilojoules to three significant digits. B) 2POCl3(g)→2PCl3(g)+O2(g), ΔH∘=572 kJ, ΔS∘=179 J/K Express the Gibbs free energy in kilojoules to three significant digits. C) At what temperature (if any) would the decomposition of POCl3 become spontaneous? Express the temperature in kelvins to three significant digits. If there is no answer, enter none.
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
Find ΔHrxn for the following reaction: 3C(s,graphite)+2O3(g)→3CO2(g) Use the following reactions with known ΔH values: C(s,graphite)+O2(g)3O2(g)→→CO2(g)2O3(g)ΔH=−393.5 kJΔH=+285.4 kJ Express the energy to one decimal place and include the appropriate units.
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?
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.8 mol ZnS and 7.5 molO2. Part A Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?
Given the following data: C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ CS2(l) + 3O2(g) → CO2(g) + 2SO2(g) ΔH = -1076.5 kJ C(s) + 2S(s) → CS2(l) ΔH = +89.4 kJ Find the ΔH of the following reaction: SO2(g) → S(s) + O2(g)
For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant. 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g) 1) 2.8 mol O2 . . . ? mol PbO 2) ? mol SO2 3) 6.0 mol O2 . . . ? mol PbO 4) ? mol SO2
Consider the following reaction. CS2(g) + 3O2(g) CO2(g) + 2SO2(g) If the volumes of all products and reactants are measured at 75°C and 1 atm, what is the total volume of products if 5.00 L of CS2 and 18.0 L of O2 are used?
For the values give for ΔH and ΔS, calculate ΔG foreach for each of the following reactions at 298 K. If the reactionis not spontaneous under standard conditions at 298 K, at whattemperature (if any) would the reaction become spontaneous? a) 2PbS(s)+3O2(g) ---> 2PbO(s)+2SO2(g) ΔH= -844kj ; ΔS = -165 J/K b)2POCl3(g)--->2PCl3(g)+O2(g) ΔH= 572kJ ; ΔS= 179 J/K
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.6 mol ZnS and 9.4 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains? Express your answer using two significant figures.