Consider the reaction, which is exothermic as written, PCl5(g)  PCl3(g) + Cl2(g).  Which of the following changes would result in the production of MORE Cl2(g)? ​ I.       adding PCl3(g) II.      removing PCl3(g) III.     reducing the volume of the container IV.     removing PCl5(g) V.       increasing the temperature VI.     increasing the volume of the container VII.    adding PCl5(g) VIII.   reducing the temperature IX.     adding a suitable catalyst

The following gases are in equilibrium in a sealed glass tube. 2 NO2 (g) = N2O4 (g) (brown) (colorless) Increasing the temperature makes the gas in the tube more intensely brown in color. Decreasing the temperature has the opposite effect. Based on this observation, the reaction shown must be... O neither exothermic nor endothermic O endothermic exothermic

the reaction of (see image) is found to have an equilibrium constant of 1.1 x 10^8 at a particular temp. what does this mean?

Consider the exothermic reaction: A (g) + B (s) → 2X (g) @ 25 °C a. Propose a change in VOLUME so that the equilibrium position shifts towards the REACTANTS. b. Propose a change in TEMPERATURE so that the equilibrium position shifts towards the PRODUCTS. c. Propose a change in [A] so that the equilibrium position shifts towards the PRODUCTS.

18. The thermochemical equation for the formation of ammonia from nitrogen and hydrogen is as follows: N2(g) + 3H2 (g) 5 2NH3 (g) AH=-92,2 kJ Given the system is initially at equilibrium, which of the following actions would cause the reaction to shift to the left? a. removing NH3 (g) b. removing H2 (g) c. decreasing the temperature d. adding a catalyst e. adding N2 (g)

The following reaction is known as the water- gas shift reaction: H2(g) + CO2(g) – – CO(g) + H20(g) for which Kc = 1.53 at a temperature of 686 •C. a. Write an equation for Kc for this reaction in terms of the reactant and product concentrations. b. If you start with only 1.50 M of H20 and 1.50 M of CO, what will the equilibrium concentrations of all four substances be? Construct an ICE table and use the value for Кс above. c. What is the value of Kp for this reaction at 686 •C? d. If the reaction were at equilibrium and then CO2 was removed, in what direction would the reaction shift to recover equilibrium?

Consider the following: N2(g)+ 3H2(g) = 2NH3(g) Ke= 6.3 × 10° What is the new K, for this reaction but I rewrite it to show the production of 1 mole of H2 and 0.333 moles of N2 from 0.666 moles of NH3? A. 2.10 x 108 B. 1.17 x 103 C. 1.36 × 103 D. 3.99 x 10-27

Thursday, December 14, 2023 4:49 PM OH CH3 Br CH3 Complete the following reaction.

For the equilibrium system below, which of the following would result in an increase in the quantity of CO(g)? 2H₂(g) + CO(g) CH3OH(g) + 92 kJ A. decreasing temperature B. decreasing the volume of the container C. adding some CH3OH D. both a and b E. both b and c 101

4. Which of the following statements is false? A. Increasing the volume of the container will couse the reaction to shift to the left. B. Decreasing the volume of the container will cause the partial pressure of N2 to increase. C. Adding an inert gas such as Neon will couse the pressure in the container to increase. D. Decreasing the partial pressure of NO will cause the partial pressure of N2 to increase. E. The addition of a catalyst will speed up the reaction but will have no effect on the position of equilibrium.