Write reaction quotient for the following reactions:a.  N2(g)  + 3H2(g) <-> 2NH3(g)b.  CO2 (g) + C (s)<-> 2CO (g)

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The following reaction is product-favored at equilibrium at room temperature. C,H2 (g) + H2 (g) → C,H4 (g) Will raising or lowering the temperature make it reactant-favored? Raising the temperature can make it reactant-favored. O Lowering the temperature can make it reactant-favored. O Neither raising nor lowering the temperature can make it reactant-favored.

■ W Chapter... G N. O LCG a Ⓒ BA H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K, and Q are within 5% of each other.) (a) 2 NH3(g) = N₂(g) + 3 H₂(g) [NH3] = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(9) N₂(g) + 3 H₂(g) What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. P (NH3) = 1.90 atm, P(N₂) = 11.65 atm, P(H₂) = 11.65 atm, K = 6.6x104 O To the right, i.e. the product-side. O It will not shift. (c) 2 SO 3(g) 2 SO₂(g) + O₂(9) What is the reaction quotient? webassign.net [SO3] = 1.65 M, [SO₂), = 1.65 M, [0₂], =…

Consider the following reaction: CO (g) + 2 H₂ (9) CH3OH (g) A reaction mixture in a 5.21 - L flask at a certain temperature initially contains 27.4 g CO and 2.36 g H₂. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (K) for the reaction at this temperature. Kc = Submit ΠΑΠ ΑΣΦ 4 Request Answer ?

An empty steel container is filled with 3.00 atm of H2 and 3.00 atm of F2. The system is allowed to reach equilibrium. If Kp = 0.450 for the reaction below, what is the equilibrium partial pressure of HF? H2(g) + F₂ (g) 2 HF (g) 2

3. Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E

Consider the following exothermic reaction, used to obtain lead from its ore:2PbS (s) + 3O2 (g) + 2CO (g) ↔ 2 Pb (l) + 2SO2 (g) + 2CO2 (g)Assume that this reaction is in equilibrium. Given the following changes to the system, will the quantity of lead increase, decrease, or remain the same?i) adding more lead sulfide.ii) Adding more carbon monoxide.iii) removing some oxygen.

4) Choose the reactions below where K and K are equal. 302 (g) = 203 (9) CO (g) + H2O (g) = CO2 (g) + H2 (9) N2 (g) + 3H2 (g) 2NH3 (g) N2 (g) + O2 (9) : 2ΝΟ ( g)