What is the equilibrium constant (in atm to three decimal places) of HBr for the following reaction if P(H₂) = P(Br₂) = 1.000 atm at 25 °C? H₂(g) + Br₂(g) = 2HBr(g) K = 0.00550 Hint: The equilibrium constant, K, is given. You should convert this to the corresponding Kp

Consider the following equilibrium process at 686. °℃: CO₂(g) + H₂(g) CO(g) + H₂O(g) The equilibrium concentrations of the reacting species are [CO]=0.0560 M, [H₂] = 0.0400 M, [CO₂]=0.0830 M, and [H₂O]=0.0430 M. Part 1 of 5 Calculate K for the reaction at 686. °C. Round your answer to 3 significant digits. с Kc- Part 2 of 5 x10 If we add CO₂ to increase its concentration to 0.510 M, what will the concentrations of all the gases be when equilibrium is reestablished? Round your answer to 3 significant digits. [CO₂] = M x10 X Ś

At 1000 K, a sample of pure NO₂ gas decomposes: 2 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium. Part 1 of 2 What is the pressure of NO? Be sure your answer has the correct number of significant digits. Part 2 of 2 atm x10 atm X What is the pressure of NO₂? Be sure your answer has the correct number of significant digits. Ś x10

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.

Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall 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. yes no ☐ atm X S

At -5.21 °C the concentration equilibrium constant K = 2.9 × 10³ for a certain reaction. Here are some facts about the reaction: • The net change in moles of gases is -1. Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, 58.0 kJ/mol of heat are released. ● Using these facts, can you calculate Kat 16. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °℃ will be bigger or smaller than Kat -5.21 °C? Yes. No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No.

Heating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24

4. Toluene, C;H8(1), is an important organic solvent. It is made industrially from methylcyclohexane, C,H14(g): C,H14(g) + heat ? 2C;H8(1) + 3H2(g) State three different changes to an equilibrium mixture of these reacting gases that would shift the reaction toward greater production of toluene. State and explain each change.

Consider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.

Consider the following equilibrium: N₂ (g) + 3H₂(g) → 2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of nitrogen (N₂) and 4.50 atm of ammonia (NH3) at 250. °C. Answer the following questions about this system: 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. OO rise fall yes no atm ☐x10 X Ś