An equilibrium is established for the exothermic reaction Br₂(g) + 5 F₂(g) = 2 BrFs (g). How would each of the following changes affect the partial pressure of fluorine at equilibrium? Adding BrF5. A) The partial pressure increases. B) The partial pressure decreases. C) The partial pressure does not change.

Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H₂O(g) + H₂(g) + CO(g) Which of the following statements is/are CORRECT? 1. Increasing the concentration of H₂(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). 2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). All statements are correct. 2 only 3 only 1 only 1 & 2 only

The oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g)   ⇋   4 NO (g) + 6 H2O (g) If the temperature is decrease, what happens to the concentration of H2O?

A sample of H,S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) = 2H2(g) + S2(g) K, = 3.85 x 10-7 0.497 atm 0.215 atm 0.793 atm 0.624 atm 0.387 atm O O O

For the reaction at equilibrium: 2 H2O (g) +2 Cl2 (g) + energy 4 HCI (g) + O2(g), If a catalyst is added to the reaction mixture. The equilibrium will shift to the left. The equilibrium will shift to the right. The position of the equilibrium will not change.

Phosphorus pentachloride decomposes at higher temperatures. PC15 (8) PCl3(g) + Cl₂(g) An equilibrium mixture at some temperature consists of 5.81 g PCI, 208.23 g/mol 4.86 g PC3, 137.33 g/mol 3.59 g Cl₂, 70.91 g/mol in a 1.00-L flask. If you add 1.31 g of Cl₂, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished? O shift left O shift right Ono shift will occur [PCI5] = mol/L

Calculating an equilibrium constant from a heterogeneous equilibrium... Calcium carbonate decomposes to form calcium oxide and carbon dioxide, like this: CaCO3(s)CaO(s) + CO₂(g) compound amount CaCO3 28.4 g CaO 21.1 g CO₂ 16.6 g At a certain temperature, a chemist finds that a 4.7 L reaction vessel containing a mixture of calcium carbonate, calcium oxide, and carbon dioxide at equilibrium has the following composition: Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 X 0/3 Ś Izabella ? 00. 18 Ar 8.