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Chemistry, 21.12.2021 15:50, WallaceHarrison123
At high temperatures, some unusual sodium oxides, Na2O, Na2O2 and NaO2 form. The equilibrium constants for the dissociation reactions of these oxides are listed below. 1 K = 2 x 10-25 2 1) Na20(s) = 2 Na(2) + 3 026) 2020) 2) Naog) = Na(2) + K = 2 x 10-5 2 K = 5 x 10-29 3) Na 02(s) = 2 Na(2) + O2(g) 4) Naoz(s) = Na(2) + 029) K = 3 x 10-14 Use the information above to predict the equilibrium constant for the reaction below. 2NaO(g) = Na 202(s) K = ? Enter your answer using scientific notation. Round the answer to one significant figure. For example 6.5 x 10^-10 should be entered as 6E-10.
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Chemistry, 21.06.2019 12:50, adrian08022
Use the standard enthalpies of formation for the reactants and products to solve for the δhrxn for the following reaction. (the δhf of c2h4 is 52.26 kj/mol, co2 is -393.509 kj/mol, and h2o is -241.818 kj.) c2h4 (g) + 3o2(g) 2co2 (g) + 2h2o(g) δhrxn = the reaction is .
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Chemistry, 22.06.2019 20:30, Schoolworkspace453
Consider the following unbalanced equation for the combustion of hexane: αc6h14(g)+βo2(g)→γco2(g)+δh2o(g) part a balance the equation. give your answer as an ordered set of numbers α, β, γ, use the least possible integers for the coefficients. α α , β, γ, δ = nothing request answer part b determine how many moles of o2 are required to react completely with 5.6 moles c6h14. express your answer using two significant figures. n n = nothing mol request answer provide feedback
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At high temperatures, some unusual sodium oxides, Na2O, Na2O2 and NaO2 form. The equilibrium constan...
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