Calculate K for the reaction of N 2 and H 2 to form NH 3 with the given balanced equation and the following equilibrium concentrations: [N 2] = 0.12 M; [H 2] = 0.36 M; [NH 3] = 1.1 M.

A gas mixture of 25% CO, 55% H₂ and 20% N₂ is fed to a reactor where methanol gas phase synthesis is carried out. The reactor in question reaches equilibrium at 623 K and 300 bar conditions based on the following reaction and equilibrium constant value. Determine the composition values of the mixture in equilibrium. CO (g) + 2 H₂ (g) CH3OH (g) K= 6.25x10-5

Conversion of cis-2-butene to trans-2-butene is represented by the equation kc=trans/Cisco. Calculate the equilibrium constant when 3mol of the cis-isomer in 8L is heated to 500 Celsius and at equilibrium the trans-ionomer is 2.1mol.

Redox/ oxidation. Someone please help!

For the reaction H₂(g) + Cl₂ (g) → 2HCl(g) AG = -191 kJ and AS = 20.0 J/K at 312 K and 1 atm. This reaction is product favored under standard conditions at 312 K. The standard enthalpy change for the reaction of 2.09 moles of H₂(g) at this temperature would be kJ.

A sample of Al (2.8 g) reacts with a sample of Cl (4.15 g) according to equation below: 2Als) + 3C12 (g) 2AIC\3(s) What is the theoretical yield of AICI; in this reaction? The mass number for Al is 27 while for Cl is 35

Find the difference between the heat of reaction at constant pressure and at constant volume for the following reaction at 25°C (assuming that it could take place)

Examine the reaction equation below. "Heat" being present on the reactant side of an equation indicates what? "Heat" + 2NH3  N2 + 3H2

In the combustion of hydrogen, the following reactions involving radicals are fast in both the forward and reverse directions.   Use the assumption of partial equilibrium to derive algebraic expressions for the molar concentrations of the three radical species, O, H, and OH, in terms of the kinetic rate coefficients and the molar concentrations of reactant and product species, H2, O2, and H2O.