Two equilibrium reactions of nitrogen with oxygen, with their corresponding equilibrium constants (Kc) at a certain temperature, are given below. reaction (1): N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 2.59e-31 reaction (2): N2(g) + 1/2 O2(g) equilibrium reaction arrow N2O(g); Kc = 3.31e-24 Using this set of data, determine the equilibrium constant for the following reaction, at the same temperature. reaction (3): N2O(g) + 1/2 O2(g) equilibrium reaction arrow 2 NO(g)

Explain how carbon monoxide can cause death

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

What reaction is taking place? 02 + c3h8 = h20 + co2