5 attempts left Check my work Enter your answer in the provided box. For the reaction N2(g) + 3H2(g) = 2NH3(g) Kp is 2.79 x 10 at 472°C. What is the K, for this reaction at 472°C?

The equilibrium reaction Fez O4(s) + 3 H2(g) 2 3 Fe(s) +4 H20(g) has AH° = 149.77 kJ/mol. Write down Shift Left, Shift Right, or No Change for each of the following situations: a) Solid Fe is added to the reaction. b) The temperature of the reaction is increased. c) The volume of the reaction vessel is suddenly doubled with no change in temperature. d) After doubling the volume of the reaction vessel, the partial pressure of H20 is tripled with no change in temperature.

2. Consider the equilibrium system: 2 NOB (g) 2 NO (g) + Br2 (g) At a 298 °K, analysis of an equilibrium mixture finds the following concentrations: [Br2] = 4.0 mol/L, [NOB1] = 0.50 mol/L, [NO] = 2.0 mol/L. Calculate Keq for the reaction at this temperature. (:

plz given correct answer with detail step by step explanation

Choose the letter of the correct answer. N204 (g) = (reversible to) 2NO2 (g), K = 4.63 x 10-3 I. the given is equation is an example of homogenous equilibrium II. Equilibrium will lie to the right Which statement(s) is/are correct?

N2(g) + 3H2 (g) = 2NH3 (g) AH°pn =-92 kJ Which of the following changes would cause the value of K for this reaction to increase? You can choose any combination of answers. Decreasing the volume of the reaction container. Heating the reaction container Cooling the reaction container Adding Helg) to the reaction container removing NH3(g) from reaction container.

At -7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction. Here are some facts about the reaction: • The constant pressure molar heat capacity C, 1.76 J·mol -1. K¯!. • If the reaction is run at constant pressure, the volume increases by 14.%. The initial rate of the reaction is 11. mol·L - 1 -1 •S O Yes. Using these facts, can you calculate K, at 15. °C? O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K at Yes, and K, will be 15. °C will be bigger or smaller than K, at -7.73 °C? smaller.

3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.

Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.