Construct the expression for Kp for the following reaction. C(s) + 2 H₂(g) → CH4(g)

(2) Nitrogen oxide is a pollutant in the lower atmosphere that irritates the eyes and lungs and leads to the formation of acid rain. Nitrogen oxide forms naturally in the atmosphere according to the endothermic reaction: N2 (g) + O2 (g) = 2 NO (g) Kp = 4.1 × 10-31 at 298 K Use the ideal gas law to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 atm and a temperature of 298 K. Assume that nitrogen composes 78% of air by volume and that oxygen composes 21% of air. Find the “natural” equilibrium concentration of NO in air in units of molecules/cm³.

Consider the following reaction and its equilibrium constant: I2(8) = 2 1(g) Kp = 0.209 A reaction mixture contains 0.89 atm I 2 and 1.88 atm I. Which of the following statements is TRUE concerning this system? The reaction will shift in the direction of reactants. The reaction quotient will rease. The reaction will shift in the direction of products. The equilibrium constant will decrease. The system is at equilibrium.

Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. KJ Now suppose a reaction vessel is filled with 9.62 atm of nitrosyl chloride (NOCI) and 4.77 atm of chlorine (C₁₂) at 722. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C1₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. O rise O fall O yes O no 0₂ atm 0 x10 X

For the reaction COCl2g(?) ↔ ?o (?) + ?l22(?), Kp was experimentally determined to be 0.0444 at 394.8 °C. assume that initially, n moles of COCl2(g) and no moles of CO(g) and Cl2(g) are present.a)  Find the partial pressures of CO (g) and Cl2 (g) at equilibrium given 1.00 bar total pressure.b)  What is the value of ∆rG at equilibrium?c)  Determine ∆?G using the given equilibrium constant K.

The value of Kp for the reaction 2 A(g) + B(g) + 3 C(g) → 2 D(g) + E(g) is 19350 at a particular temperature. What does the magnitude of Kp tell us about the equilibrium position of the reaction? A) There are many more products than reactants. B) There are only a few more products than reactants. C) There are many more reactants than products. D) There are only a few more reactants than products. +

Consider the following equilibrium: N₂O4 (g) → 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O rise fall yes no atm x10 X 5

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 2.0 L reaction vessel contained a mixture of 1.0 mol Fe, 1.0 × 10⁻³ mol O₂, and 2.0 mol of Fe₂O₃ at 2000 °C. What are the values of Kc and Kp for this reaction?   4 Fe(s) + 3 O₂(g) ⇌ 2 Fe₂O₃(s)   Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.

Calculate K for the reaction at 511 K: SO2Cl2(g) = SO2(g) + Cl2(g) Kp= 3.08 x 10 If the answer is 2.5 x 10, ,express the answer as 2,5E-2.

Using the equilibrium constants for the reactions below: 4CO(g) + 20(s) + 2CO2 (g) Kp = 5.92 x 10-29 COCI2(g) → CO(g) + Cl2(g) Кр- = 167 Find the equilibrium constant Kp for the following reaction: C(s) + CO2(g) + 2C12(g) → 2COCI2 (g) Enter the number with the correct number of sig figs. For a scientific notation, enter as #e# without any spaces, where e means "10 to the power of"