A mixture of 0.10 molmol of NONO, 0.050 molmol of H2H2, and 0.10 molmol of H2OH2O is placed in a 1.0-LL vessel at 300 KK. The following equilibrium is established: 2NO(g)+2H2(g)←→N2(g)+2H2O(g)2NO(g)+2H2(g)←→N2(g)+2H2O(g) At equilibrium [NO]=0.062M[NO]=0.062M. A. Calculate the equilibrium concentration of H2H2. Express your answer using two significant figures.   B. Calculate the equilibrium concentration of N2N2. Express your answer using two significant figures.   C. Calculate the equilibrium concentration of

A mixture of 0.009482 mol of CH4, 0.02708 mol of H2S, 0.02785 mol of CS2, and 0.02860 mol of H2 is placed in a 1.0-L steel pressure vessel at 3918 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) At equilibrium 0.001533 mol of CH4 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4).Peq(H2S).Peq(CS2).Peq(H2).(b) Calculate KP for this reaction.KP.

The equilibrium constant, Ke, for the following reaction is 1.80x104 at 298 K. NH4HS(s) =NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.457 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] = M %3D

Consider the following reaction where Kc PC15 (9) PC13 (g) + Cl₂ (9) A reaction mixture was found to contain 0.117 moles of PC15 (g), 0.0259 moles of PC13 (g), and 0.0368 moles of C1₂ (g), in a 1.00 liter container. Calculate c Qc² = = 0.0120 at 500 K. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? O The reaction must run in the forward direction to reach equilibrium. O The reaction must run in the reverse direction to reach equilibrium. O The reaction is at equilibrium.

help  -write the expression for equilibrium constant kp for the following reaction 4clo2(g) ==2cl2o(g)+3o2(g)

Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1   2 Co3O4(s)   ↔   6 CoO(s) + O2(g)

The following equilibrium constants were determined at 1123 K: Kp=7.79 × 10 Kp"=1.67 × 10² 2CO(g)C(s) + CO₂(g) COC1₂(g) CO(g) + Cl₂ (g) Part 1 of 2 Calculate the equilibrium constant at 1123 K for the reaction: 2COC1₂ (g) C(s) + CO₂(g) + 2Cl₂ (g) Round your answer to 3 significant digits. Part 2 of 2 n x10 = Kp² X Write the equilibrium constant expression: X Olo 15