The value of Kc for the interconversion of butane and isobutane is 2.5 at 25°C. If you place 0.019 Mol of butane in a 0.50 l flask at 25°C and allow equilibrium to be established, what will the equilibrium concentrations of the two forms of butane?

Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO,(9) + 0,(9) → 2 SO3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide has the following composition: compound concentration at equilibrium SO2 0.78M O, 1.5M SO3 0.94M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Calculating an equilibrium constant from a partial equilibrium composition Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 500. mL flask with 3.3 atm of ammonia gas and 0.87 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.6 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P ☐ x1 x10 ☑ 5

Nitrogen dioxide decomposes according to the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g)  Where Kp = 4.48 x 10 ^ -13 at a certain temperature. If 0.40 atm of NO is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO (g) and O2 (g)?  P NO =   atm NO P O2 =   atm O2 Use correct significant figures.

The equilibrium constant, Ke, for the following reaction is 7.00 x 10-5 at 673 K. to access important values if needed for this question. NH₂I(s) ⇒ NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.33 L container at 673 K contains 1.71 mol of NH₂I(s) and 0.445 mol of NH3, the number of moles of HI present is mol.

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

A student ran the following reaction in the laboratory at 675 K: H2(g) + I2(g) 2HI(g) When she introduced 0.226 moles of H2(g) and 0.248 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.11×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =

Carbon monoxide and water vapor are formed when carbon dioxide and hydrogen react. CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium constant for the reaction is KC = 2.78 at 167 ℃. If 0.787 mol of carbon dioxide is added to 0.911 mol of hydrogen in a 1.87–L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of carbon monoxide?

Calculating an equilibrium constant from a partial equilibrium composition Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 2.0 L flask with 1.2 atm of ammonia gas and 3.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.3 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = [] P x10 X ? olo 18 Ar 8.