**Chemical Reaction Analysis:** Consider the chemical reaction: \[ \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \] If the concentration of the reactant \(\text{H}_2\) was increased from \(1.0 \times 10^{-2} \, \text{M}\) to \(2.5 \times 10^{-1} \, \text{M}\), calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. **Use this information to answer Questions 3, 4, and 5:** The equilibrium constant (K) of the reaction below is \(K = 6.0 \times 10^{-2}\), with initial concentrations as follows: - \([\text{H}_2] = 1.0 \times 10^{-2} \, \text{M}\) - \([\text{N}_2] = 4.0 \, \text{M}\) - \([\text{NH}_3] = 1.0 \times 10^{-4} \, \text{M}\) \[ \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) \]

Steam reforming of methane ( CHA) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 75.0 L tank with 34. mol of methane gas and 14. mol of water vapor, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 4.2 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K.- Explanation Check 2021 McGraw H E MacBook Air F10 F7 esc F3 F2 * # 2$ & @ 7 8

Consider the following reaction: C₂H4(g) + H₂O(g) = C₂H5OH(g) Kc = 9.0 × 10³ At equilibrium the concentration of C₂H4 is 1.69 M and C₂H5OH 0.150 M. Determine the equilibrium concentration of H₂O(g). 1.0 × 105 M 9.9 × 10-6 M 2.8 x 10-6 0.013 M

At a particular temperature 8.0 mol NO2 gas is placed in a 1.0-L container. Over time the NO2 decomposes to NO and O2: 2NO2(g) 2 2NO(g) + O2(g) At equilibrium the concentration of NO(g) was found to be 1.8 mol/L. Calculate the value of K for this reaction (using units of mol/L for the concentrations). K =

1. At 100 C the equilibrium constant, Kc is 4.6 x 10° for the reaction, CO (g) + Cl₂ (g) = COC1₂ (g). If 0.20 moles of COCl2 is placed in a 10.0 liter container, what is the concentration of all species at equilibrium?

Consider the equilibrium system described by the chemical reaction below For this reaction, Kc = 2.4 x 10 at a particular temperature. If the equilibrium concentrations of H2O and Hz are 0.11 M and 0.019 M, respectively, determine the concentration of Oz at equilibrium. 2 H.O(g) = 2 H2(g) + On(g) NEXT If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms. Ke = 2.4 x 10 3 O RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11F [0.019 [2x]

Use the information below to answer Questions 3, 4, and 5:The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 10-2 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N2(g) + 3H2(g) ⇌ 2NH3(g) N2(g) + 3H2(g) ⇌ 2NH3(g)  3. If the concentration of the reactant H2 was increased from 1.0 x 10-2 M to 2.5 x 10-1M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift by comparing the value of Q to K.   4. If the concentration of the reactant H2 was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift by comparing the value of Q to K..   5. If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift by comparing the value of Q to K..

3. Phosgene gas decomposes according to the following reaction. If a sample of phosgene gas at an initial concentration of 0.500 M is heated at 527°C in a reaction vessel, the concentration of carbon monoxide at equilibrium is 0.046 M. Calculate the equilibrium constant for the reaction at 527°C. COCl2(g) CO(g) + Cl2(g) + 4. The equilibrium constant for the following equation is Kc = 0.11. Calculate the equilibrium concentrations of ICI (g), 12(g), and Cl2(g) when 0.65 moles of 12(g) and 0.33 moles of Cl2(g) are mixed in a 1.5-liter reaction vessel. 2 ICI(g) 12(g) + Cl2(g)

Consider the following reaction: A(g) = 3 B(g) A reaction mixture initially contains 1.3 M of A. Determine the equilibrium concentration of B if Kc for the reaction at this temperature is 8.62 x 10. Calculate this based on the assumption that the x value is negligible compared to 1.3.

Consider the decomposition of nitrosyl bromide into nitrogen monoxide and bromide gas, which has an equilibrium constant Kc = 6.2 x 10-5 when the reaction occurs at a certain temperature.  If the initial concentration of nitrosyl bromide is 0.832 M, what will be the equilibrium concentration of nitrogen monoxide gas? 2 BrNO (g) <---> 2 NO (g) + Br2 (g)