Consider the following reaction: CO (g) + 2 H₂ (9) = CH3OH (9) An equilibrium mixture of this reaction at a certain temperature was found to have [CO] = 0.115 M, [H₂] = 0.118 M, and [CH3OH] = 0.185 M. What is the value of the equilibrium constant (K) at this temperature? K₂= Submit ΠΙ ΑΣΦ 5 Request Answer ?

A student ran the following reaction in the laboratory at 1080 K: 2SO3(g) 2S02(g) + O₂(g) When he introduced SO3(g) at a pressure of 0.886 atm Into a 1.00 L evacuated container, he found the equilibrium partial pressure of SO3(g) to be 0.340 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer 44 $ T R F V/ % 5 Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 G ^ 6 MacBook Air Y H & 7 RN U * 0 J ► 11 F8 M ( 9 ►► K F9 O 1 F11 + { Save and Exit = F12 11

Consider the following reaction: SO2Cl2 (g) SO2 (g) + Cl2 (g) A reaction mixture is made containing an initial [SO₂Cl₂] of 2.2x10-2 M. At equilibrium, [C1₂] = 1.1x10-² M. Calculate the value of the equilibrium constant (Kc). Express your answer using two significant figures. ΓΙ ΑΣΦ Kc = Submit Request Answer ?

For the reaction below, the concentrations at equilibrium are [SO₂] = 0.60 M, [O₂] = 0.25 M, and [SO₂] = 1.6 M. What is the value of the equilibrium constant, Ke? 2 SO₂(g) + O₂(g) →→→ 2 SO₂(g) • Report your answer using two significant figures. Provide your answer below: