The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. Which of the following actions will decrease the value of the equilibrium constant, Kc? NaOH(s) + CO2(g) ⟷⟷ NaHCO3(s)     ΔH°rxn < 0 Group of answer choices Increase the temperature. Add N2 gas to

Consider the following reaction at equilibrium taking place in the gas phase: H2   +   I2   double arrows   2 HI In what direction will the equilibrium shift if the volume of the container is decreased?     Towards reactants     Towards products     Neither

The following reaction is exothermic. 2 NO(g) + 2 H2(g) ⇔ N2(g) + 2 H2O(g) In which direction does the equilibrium shift as a result of each of the following changes? Here are the possible answers: to the right, to the left, no effect Place these actions in chronological order. Space 1: The hydrogen gas is removed. Space 2: The gas pressure in the reaction vessel is increased by decreasing its volume. Space 3: The gas pressure in the reaction vessel is increased by pumping argon gas into it while keeping the volume constant. Space 4: We raise the temperature. Space 5: A catalyst is used.

An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) ⇒ CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂ I mol

14.  The following reaction is allowed to come to equilibrium and then the volume is increased.  Predict the effect of the indicated volume change once equilibrium is restored.                         H2O(g)            +          CO2(g)               double arrow              H2CO3(g)     The reaction will shift right.     The reaction will shift left.     There will be no effect.     Effect can not be determined from information provided.

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(s) At a certain temperature, a chemist finds that a 7.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 7.0 g O2 5.8 g HgO 16.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10

Consider the equilibrium below.2 Cl₂ (g) + 2 H₂O (g) ⇄ 4 HCl (g) + O₂ (g)At a certain temperature, a container is fill with Cl₂ and H₂O gases until the pressures of Cl₂ = 2.000 atm and the pressure of H₂O = 4.000 atm. When equilibrium is reached, the total pressure in the container is 6.982 atm. Calculate the value of the equilibrium constant Kp at this temperature.Very large or very small numbers should be entered in scientific notation using the 'E' format, just like your calculator. A number such as 2.34×10-7 should be entered as 2.34E-7Kp=

An evacuated reaction vessel is filled with 0.800 atm of N₂ and 1.681 atm of Br2. When equilibrium is established according to the reaction below, there are 1.425 atm of Br2 remaining in the vessel. What is the equilibrium partial pressure of NBr3? 2 NBr3 (g) = N₂ (g) + 3 Br2 (g)

60) The following are the values of the equilibrium constant, K, for four different chemical reaction systems. For each of the chemical reaction systems, describe the equilibrium position of the given temperature as mostly products, mostly reactants, or equal concentrations of reactants and products. a) K= 10-12 at 25 °C

Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) → Fe₂O3(s)+ 3 H₂(g) At a certain temperature, a chemist finds that a 2.5 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound Fe H₂O Fe₂O3 H₂ amount 4.04 g 2.87 g 3.49 g 2.08 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. C K = 0 C Dx1 x10 X Ś