ta given temperature, the equilibrium constant K, for the reaction below is 2.68×10*3. eso,g) +0,(g) 250, (g) Vhat is the value of the equilibrium constant for each of the following reactions at that temperature? so,(e) + -0,6) – so,6) 2s0, (g) 2s0,4) + 0,(g) so, (G) – so,4) + 0,4)

At a certain temperature, the reaction PCl5(g) <====> PCl3(g) + Cl2(g) has an equilibrium constant Kc=5.8x10^-2    a) calculate Kc for the synthesis of 2 moles of PCl5(g) at the same temperature

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 × 10-4 at a certain temperature. If a solid sample of CaCro4 dissolves in solution, what will the equilibrium concentration of Ca2* in the solution be? СacrOa(s) 3D са?" (аq) + CrO,? (aq) 2- 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. CaCrO4(s) Ca²*(aq) CrO,2 (aq) + Initial (M) Change (M) Equilibrium (M)

At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases.   At this temperature, K=0.0169 . What are the partial pressures at equilibrium of the hydrogen and iodine if initially a sealed flask at 800 K contains only HI  at a pressure of 0.242 atm?

The following reaction is exothermic. 2 NO(g) + 2 H2(g) ⇔ N2(g) + 2 H2O(g) In which direction does the equilibrium shift as a result of each of the following changes? Here are the possible answers: to the right, to the left, no effect Place these actions in chronological order. Space 1: The hydrogen gas is removed. Space 2: The gas pressure in the reaction vessel is increased by decreasing its volume. Space 3: The gas pressure in the reaction vessel is increased by pumping argon gas into it while keeping the volume constant. Space 4: We raise the temperature. Space 5: A catalyst is used.

The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =

At a given temperature, the equilibrium constant Kc for the reaction below is 2.37x103. 2S0, (g) +0,(g) – 2SO3 (g) What is the value of the equilibrium constant for each of the following reactions at that temperature?

Kc = 0.76 at a given temperature for the reaction: 2 HI (g) = H2 (g) + l2 (g) . Consider the condition [HI] = 0.36 M and [H2] = [12] = 0.60 M. Which of the following statements is correct? a) The quotient Q > Kc. b) The reaction will shift to right to establish equilibrium. O a) only O b) only Both a) and b) are correct. neither a) nor b) is correct.

Consider the reaction, 2AB2(g) = A2(g) + 2B2(g), Kc = 0.263 at 25°C. The reaction begins with an unknown concentration of AB2 in the reaction flask. At equilibrium, the concentration of AB2 is found to be 0.00545 M. a) Complete the ICEE table below, b) Write the equilibrium expression and equation for this reaction (pay close attention to coefficients!), c) Calculate the equilibrium concentration of both products, and d) Calculate the initial concentration of AB2. You should confirm that your equilibrium concentrations will give the correct equilibrium constant when plugged into the expression. ICEE table I C E 2 AB₂(g) A₂(g) + 2 B₂(g)

Question 4 of 25 Submit The equilibrium constant for the reaction 2 HF (g) = H2 (g) + F2 (g) is 0.270 at a particular temperature. What is the equilibrium constant for the equation ½ H2 (g) + ½ F2 (g)= HE (g)? 1 3 C 7 9. +/- x 10 0 LO 00