Construct the expression for Ksp for solid Ba3(PO4)2 in aqueous solution. Вaз(РOд)2(s) 3 З Ва" (aq) + 2 РО," (aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, use the tiles to form the expression. Ksp II

Hydrogen and chlorine react to form hydrogen chloride, like this: H₂(g) + Cl₂(g) - 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound concentration at equilibrium H₂ 0.26M Cl₂ HCI Kc Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. = 1.4M 0 0.97 M 0 x10 X

Consider the reaction: CH3COOH (aq) + H₂O(1) K = 1.8 x 10-5 at 25 °C Part A If a solution initially contains 0.225 mol L-¹ CH3COOH, what is the equilibrium concentration of H3O+ at 25 °C? Express your answer in moles per litre to two significant figures. 15. ΑΣΦ [H3O+] = H3O+(aq) + CH3COO (aq) Submit Request Answer ? mol L-1

Chapter 12 part 1 #12

3. Given the chemical reaction A(aq) + 2B(aq) → C(aq) + 3D(aq) Initially, you have 2 moles of A and 3 moles of B dissolved in a total volume of 3 L. a. X moles of A reacted, and the solution reached equilibrium. Solve for the End state in term of x b. Write down the expression of the equilibrium constant (Keq) in term of x and volume.

Part B The reaction will proceed toward 1-butene to reach equilibrium. Determine the partial pressures of 1-butene and isobutene. 1-butene = 2.6 bar. P isobutene = 2.1 bar 1-butene = 2.1 bar, P isobutene = 2.6 bar OP, 1-butene = 2.2 bar, P = 1.7 bar isobutene O P. = 2.7 bar, P = 2.2 bar 1-butene isobutene

The equilibrium constant K₁, K2 and K3 for the reactions below are S(s) + O₂(g) → SO₂(g), K₁ = 4.2 × 1052 2S (s) +30₂(g)2SO3(g), K₂ = x 2SO2(g) + O2(g)2SO3(g), The value of K₂ is 9.8 × 1028 2.6 × 1075 □ 6.7 × 10¹2 1.34 × 1032 9.8 x 10128 K3= 5.6 x 1023

At 454 K, Al,Cl6(g) reacts to form Al;Cl,(g) according to the equation 3 Al,Cl,(g) = 2 Al;Cl,(g) In an experiment at this temperature, the equilibrium par- tial pressure of Al,Cl(g) is 1.00 atm and the equilibrium partial pressure of Al;Cl,(g) is 1.02 × 10-2 atm. Compute the equilibrium constant of the preceding reaction at 454 K.

At 503 K the equilibrium constant K. for the dissociation of N,O4, N204(g) 2 2 NO2(g) has the value K = = 40.0. Calculate the concentration of N204 left undissociated when 1.00 mol of this gas is heated to 503 K in a 10.0 L container.

Write the equilibrium expression for the following: I2(s) + 3XeF2(s) ↔↔ 2IF3(s) + 3Xe(g)