Consider the following reaction: 2 H2O(g) + 2 SO2(g) ⇌ 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 1.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6.

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g)   1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms   2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown.   3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown.   4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.

Consider the following reaction between nitrogen and oxygen and its equilibrium constant at 2000 °C: N2(g) + O2(g) ⇌ 2 NO(g)Kc = 4.10 × 10−4 a)Is the formation of nitrogen monoxide favored at 2000 °C? Explain your answer without doing a calculation. b)What is the nitrogen monoxide concentration when a mixture of 0.40 mol of nitrogen gas and 0.30 mol of oxygen gas reaches equilibrium in a 2.0-L container at 2000°C?

4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)