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SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2]
Without knowing concentrations, one cannot calculate the actual value of Keq.
Keq=[SO3][SO2] /[SO2][NO2]
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What is the equilibrium constant for the reaction SO2(g) plus NO2(g) --- SO3(g) plus NO(g)?
The equilibrium constant for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) is given by the expression Kc = [SO3][NO]/[SO2][NO2], where square brackets denote molar concentrations. The numerical value of this equilibrium constant would depend on the specific conditions of the reaction.
How would the equilibrium change if NO2 were added to SO2(g) NO2(g) NO(g) SO3(g) heat?
The amount of NO2 and SO2 eould
The equilibrium constant for the reaction below is 31.25 at equilibrium so2 0.03 o2 0.05 and h2s 0.15 what is the equilibrium concentration of H2O?
The equilibrium constant expression for the reaction is Kc = [H2O]^2/[SO2][O2]. Given the concentrations at equilibrium, we can solve for [H2O]. Plugging in the values, we get 31.25 = [H2O]^2 / (0.03)(0.05). Solving for [H2O] gives us [H2O] = sqrt(31.25 * 0.03 * 0.05), which is approximately 0.275M.
What is the full form of so2 and no2?
SO2 stands for sulfur dioxide and NO2 stands for nitrogen dioxide.
Equation to show NO2 acts as a reducing agent and oxidising agent?
Reduction reaction: 2NO2 + 2H+ + 2e- -> N2O4 + H2O Oxidation reaction: 2NO2 -> N2O5 + e-
What is the equilibrium constant for the reaction SO2(g) plus NO2(g) --- SO3(g) plus NO(g)?
The equilibrium constant for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) is given by the expression Kc = [SO3][NO]/[SO2][NO2], where square brackets denote molar concentrations. The numerical value of this equilibrium constant would depend on the specific conditions of the reaction.
What is the equilibrium constant for the reaction SO2 plus NO2--SO3 plus NO?
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
What is the equilibrium constant for the reaction SO2(g) plus NO2(g) SO3(g) plus NO(g)?
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
How would the equilibrium change if NO2 were added to SO2(g) NO2(g) NO(g) SO3(g) heat?
The amount of NO2 and SO2 eould
The equilibrium constant for the reaction below is 31.25 at equilibrium so2 0.03 o2 0.05 and h2s 0.15 what is the equilibrium concentration of H2O?
The equilibrium constant expression for the reaction is Kc = [H2O]^2/[SO2][O2]. Given the concentrations at equilibrium, we can solve for [H2O]. Plugging in the values, we get 31.25 = [H2O]^2 / (0.03)(0.05). Solving for [H2O] gives us [H2O] = sqrt(31.25 * 0.03 * 0.05), which is approximately 0.275M.
How would the equilibrium change if SO3 were added to SO2(g) plus NO2(g) NO(g) plus SO3(g) plus heat?
The amount of NO and SO3 would increased.
What is the full form of so2 and no2?
SO2 stands for sulfur dioxide and NO2 stands for nitrogen dioxide.
What is Keq for the reaction 2SO2 g O2 g 2SO3 g?
keq= [SO2]2[O2]/[SO3]2
Equation to show NO2 acts as a reducing agent and oxidising agent?
Reduction reaction: 2NO2 + 2H+ + 2e- -> N2O4 + H2O Oxidation reaction: 2NO2 -> N2O5 + e-
What would the equilibrium concentration of NO be in a gas mixture that contains 1.7 M SO3 0.070 M SO2 and 1.3 M NO2 if Keq 10.8 at those conditions?
SO3 + NO SO2 + NO21.7M + xM |=| 0.070M + 1.3MKeq = 10.8 = [SO2]*[NO2] / [SO3]*[NO] = 0.070*1.3 / 1.7*xSolving x (concentration NO at eq.) 10.8 * (1.7*x) = 0.070*1.3x = 0.0091 / 18.36 = 0.000496 = 0.00050 M = 0.50 mM
What is a major factor that is responsible for acid rain?
NO2 and SO2
Which gas is affecting Taj mahal?
Nitrogen and Sulphur gases such as NO2 and SO2 are affecting Taj Mahal in getting yellowish.
