Consider the following reaction: SO2 + 2 H2S → 3 S + 2 H2O If 7.40 g of SO2 reacts via this reaction in excess H2S, what mass (in g) of H2O will be produced?
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Consider the following reaction: SO2 + 2 H2S → 3 S + 2 H2O If 7.40...
Consider the following reaction: 2 H2O(g) + 2 SO2(g) ↔ 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6. Consider the following reaction: 2 H2O(g) + 2 SO2(g) ↔ 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc...
The following reaction occurs within an erupting volcano: 2 H2S(g) + SO2(g) 3 S(s) + 2 H2O(g) At 650 K, an equilibrium mixture contained H2S, SO2, and H2O at partial pressures of 1.17 atm, 1.07 atm, and 0.83 atm respectively. Calculate Kp at 650 K for the reaction
Consider the following reaction: 2H2S(g)+SO2(g)⇌3S(s)+2H2O(g) A reaction mixture initially containing 0.480 M H2S and 0.480 M SO2 was found to contain 1.0×10−3 M H2O at a certain temperature. A second reaction mixture at the same temperature initially contains [H2S]= 0.255 M and [SO2]= 0.325 M . Calculate the equilibrium concentration of H2O in the second mixture at this temperature. Express your answer using two significant figures.
Consider the following unbalanced chemical equation H2S(g)+O2(g)=SO2(g)+H2O(g) Determine the maximum number of moles of SO2 produced from 10.00 moles H2S and 5.00moles of O2
Consider the following unbalanced chemical equation. H2S(g) + O2(g) → SO2(g) + H2O(g) Determine the maximum number of moles of SO2 produced from 10.0 moles of H2S and 4.00 moles of O2.
Consider the reaction below Al2S3(s) + H2O(l) → Al(OH)3(s) + H2S(g) If 15.0g of aluminum sulfide and 10.0g of water are allowed to react as above, and assuming a complete reaction a. by calculation, find out which is the limiting reagent. b. calculate the maximum mass of H2S which can be formed from these reagents. c. calculate the mass of excess reagent remaining after the reaction is complete.
34. At volcanic sites, sulfur is formed via the following reaction. 2 H2S(g) +SO2(g) = 3S(s) +2 H20(g) a. Calculate the equilibrium constant, K, for this reaction at 25°C. 4 Gº (kJ/mol H2S (8) SO2) H20 (8) -33.0 -300.4 -228.6 s, b. Predict whether sulfur formation becomes more or less favorable as temperature increases. Explain. C Sulfur dioxide is a pollutant released by power plants. Would this reaction be suitable for removing SO2 from power plant waste?
4. Balance the following chemical reaction: H2S(0) + O2(g) → SO2(g) + H2O
When H2S(g) reacts with H2O(l) to form H2(g) and SO2(g) , 70.5 kcal of energy are absorbed for each mole of H2S(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) Compound ΔHof (kJ/mol) Sof (J/mol.K) H2S(g) -20.6 205.8 O2(g) 0 205.2 H2O(l) -285.8 70.0 SO2(g) -296.8 248.2 1.Calculate ΔHrxn. 2.Calculate ΔSsurroundings. 3Calculate ΔSuniverse.