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1) Consider the following reaction of hydrogen sulfide with oxygen gas to form sulfur dioxide and...
1) Consider the following reaction of hydrogen sulfide with oxygen gas to form sulfur dioxide and hydrogen gas HS + O2(g) SO2(g) +H219) a) If AH = -276.73 kJ/mol and AS --31.52 1/(mol*K), what is the equilibrium constant (K) at 8500. K? You will have to solve for AG first. b) 250.0 mmol of HS and 250.0 mmol of Oz were placed in a 1.250 L flask at 8500. K. What are the equilibrium concentrations of all species? c) What...
please show work Hydrogen sulfide reacts with oxygen to give sulfur dioxide and water according to the following balanced equation: 2 H2S (g) + 3 O2(g) 2 SO2(g) + 2 H20 (8) If we allow 8.52 g of hydrogen sulfide (H2S) to react with an ex a) Calculate the number of moles of SO2 that can be produced from b) Calculate the mass in grams of SO2 that can be produced from znat can be produced from this reaction: ac...
Hydrogen sulfide and oxygen react to form sulfur dioxide and water, like this: 2 H,S(o)+302(9)-2S0(9)+2H,0(9) Use this chemical equation to answer the questions in the table below. None. Suppose 65.0 mmol of H2S and 97.5 mmol of O, are added to an Some, but less than 65.0 mmol. empty flask. How much H,S will 65.0 mmol. in the flask at equilibrium? Suppose 150. mmol of So2 and 150. mmol of H20 are added to an empty flask. How much H2S...
For the following reaction, 6.19 grams of hydrogen sulfide are mixed with excess oxygen gas. The reaction yields 2.75 grams of water. hydrogen sulfide (g) + oxygen (g) water (l) + sulfur dioxide (g) What is the theoretical yield of water ? grams What is the percent yield of water ? %
I need help in hurry, please Sulfur dioxide (SO2) and hydrogen sulfide are toxic byproducts of many industrial processes. To prevent their release to the environment, they can be neutralized to form elemental sulfur through the Claus process, which follows the reaction: 2H2S + SO2 + 2H20 + 35 You have been tasked with neutralizing sulfur dioxide and hydrogen sulfide in a continuous reactor. The reagents arrive in stoichiometric proportion at 250°C and 100 kPa. The feed flowrate is 10...
Sulfur trioxide is formed from sulfur dioxide and oxygen according to the reaction formula 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) with the equilibrium constant 2.5 × 1010 at the temperature 5.0 × 102 K. A reaction vessel with a volume of 0.25 L contains from start 0.030 moles of SO2 (g) and 0.050 moles of O2 (g). a) Calculate the partial pressure SO3 (g) after equilibrium is reached at 5.0 × 102 K. b) Will more...
Hydrogen sulfide (H2S)reacts with oxygen (O2) to produce sulfur dioxide (SO2) and water. How many grams ofSO2will be produced if 100 g of H2Swas reacted with 100 g ofO2? (restrict your answer to 4 significant figures) Type your response
The reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g) proceeds as follows: 2H2S(g) + 302(g) 2H2O(g) + 2802(g) When 12.9 grams of H2S(g) react with sufficient O2(g), 197 kJ of energy are evolved. What is the value of AH for the chemical equation given? kJ
1. In the gas phase, sulfur dioxide reacts with oxygen to form sulfur trioxide, 2502 + O2 = 2503. An equilibrium mixture at 1000K and 1767 torr had the following mole fractions: x(SO2) = 0.310, x(O2) = 0.250. SO3 was also present. Calculate Koº and AG° at 1000K, assuming all gases behave ideally.
Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide 2H, S(g) + 302(g) → 2802(g) + 2H2O(g); AH = -1036 kJ Calculate the enthalpy change to burn 36.5 g of hydrogen sulfide. CkJ Submit Answer Try Another Version 8 item attempts remaining