10.) Hydrogen sulfide (H2S) is a contaminant commonly found in natural gas. It isremoved by reaction with oxygen to produce elemental sulfur. 2H2S(g) + O2(g)= 2S(s) + 2H2O(g) For each of the following scenarios, determine whether the equilibrium will shift to the right, shift to the left, or neither: (a) addition of O2(g) (b) removal of H2S(g) (c) removal of H2O(g) (d) addition of S(s).

3. Please don't write on a paper. I can't understand handwritten.

Iron and water react to form iron (III) oxide and hydrogen, like this: 2 Fe(s)+3 H₂O(g)→Fe₂O3(s)+ 3 H₂(9) At a certain temperature, a chemist finds that a 8.1 L reaction vessel containing a mixture of iron, water, iron (III) oxide, and hydrogen at equilibrium has the following composition: compound amount Fe 1.92 g H₂O 1.12 g Fe₂03 2.32 g H₂ 2.30 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 X

At 500K, the methanol decomposes according to the following reaction, CH3OH(g) = CO(g) + 2 H2(g) K= 9.60×10-2 Some methanol, CH3OH (molar mass: 32 g/mol), is placed into a rigid 2.00-L vessel, and the temperature is raised to 500K. If the concentration of H2 in the equilibrium mixture is 0.246M, what is the initial concentration of methanol? O A, 0.231 M Ов. 0.866 М OC 0.200 M OD. 1.109 M O E. 0.012 M

Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ

Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 1 atm of NOBr is sealed in a flask. At equilibrium, the partial pressure of NOBr is 0.82atm.  What is the equilibrium constant, Kp, for the reaction?

1. 2.00 moles of ammonia are heated in a sealed 1.00 L container at 650°C. At this temperature, ammonia decomposes to nitrogen and hydrogen gas. 2 NH3 (g) = N2 (g) + 3 H2 (g) At equilibrium, the concentration of ammonia in the container is 1.00 M. What is the value of Ke for this reaction at 650°C?

3. For the following reaction at equilibrium, 2BrNO(g) → 2NO(g) + Br2(g), what will happen if the volume of the container is decreased? (a) The reaction remains unchanged (b) The reaction will shift to the left (c) The reaction will shift to the right

At a given temperature, the equilibrium constant K, for the reaction below is 2.68×10¯³. 2s0,(g) +02(g) 2so, (g) What is the value of the equilibrium constant for each of the following reactions at that temperature? so,) + 0,) – so,() 250, (2). - 250, (g) + 0,(g) so, )

demonstrate an understanding of the concept of dynamic equilibrium and the variables that cause shifts in the equilibrium of chemical systems.