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Consider the following mixture of SO2(g) and O2(g).If SO2(g) and O2(g) react to form SO3(g),draw a representation of the product mixture assuming the reaction goes to completion. What is the limiting reactant in the reaction? If
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At 900 K the following reaction has Kp=0.345; 2 SO2(g) + O2 (g) -> 2 SO3 (g) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.145 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3
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Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. (See the appendix. Enter your answer to the tenth place.) (a) 2 H2S(g) + 3 O2(g) 2 H2O(l) + 2 SO2(g) (b) N2O4(g) + 4 H2(g) N2(g) + 4 H2O(g) (c) SO2(g) +
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Sulfur trioxide decomposes into sulfur dioxide and oxygen in an equilibrium. You have a 3.00 L vessel that is charged with 0.755 mol of SO3. At equilibrium, the amount of SO3 is 0.250 mol. 2 SO3 (g) ----> 2 SO2 (g) +O2 (g) A)
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What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the following reaction in each of the following cases? 2 SO3(g) equilibrium reaction arrow 2 SO2(g) + O2(g) ΔH° = 197 kJ (a) Oxygen gas is removed.
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What would be more acidic? SO2 or SO3? Does this have to do something with the higher oxidation state? And why is that? Or can we say SO3 is more acidic by, SO2+H2O--->H2SO3 SO3+H2O--->H2SO4 as H2SO4 is more acidic?
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chemistry
Given the thermochemical equation SO2(g) + ½ O2(g) ---> SO3 (g) DH = -99.1 kJ calculate the enthalpy change (DH) when 89.6 g of SO2 is converted to SO3. 1. 69.3 kJ 2. -111 kJ 3. -139 kJ 4. 139 kJ 5. -69.3 kJ help plz
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Data: SO2(g)+ 1/2O2(gas)forms SO3(g)Delta H = -99.1 kJ. Given the above data, calculate the enthalpy change when 89.6 g of SO2 is converted to SO3. Is this a grams to moles conversion or what? I can't find any examples of this
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Science
Given the following balanced equation, determine the rate of reaction with respect to [O2]. 2 SO2(g) + O2(g) → 2 SO3(g)
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Calculate the change in heat for the reaction SO2 + 1/2O2 --> SO3
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An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the
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At a certain temperature, the equilibrium constant Kc is 0.154 for the reaction 2 SO2(g) + O2(g) *) 2 SO3(g) What concentration of SO3 would be in equilibrium with 0.250moles of SO2 and 0.578 moles of O2 in a 1.00 liter container
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