Initial (M) Change (M) Equilibrium (M) -2.0 Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H₂, 8.0 M N2, and 4.0 M NH3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 0 2.0 5.0 N₂(g) + 3 H₂(g) = 2 NH3(g) -5.0 N₂(g) 8.0 1 6.0 4.0 -6.0 3 H₂(g) -4.0 10.0 2 NH,(9) RESET 11.0

Consider the following equilibrium system: PCI5(9) PC13 (9) + Cl₂(g) A 10.00 L evacuated flask filled with 0.4163 mol PCI5 (9) at 297.5 K. The temperature is then raised to 503.5 K, where the decomposition of PCIs gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask atm. What is the value of the equilbrium constant in terms of concentrations, Ko at 503.5 K? Kc =

A mixture of water and graphite is heated to 600 K. When the system comes to equilibrium it contains 0.13 mol of H2, 0.13 mol of CO, 0.43 mol of H2O, and some graphite. Some O2  is added to the system and a spark is applied so that the H2 reacts completely with the O2. Find the amount of CO in the flask when the system returns to equilibrium.

The equilibrium constant, K, for the following reaction is 3.78E-2 at 530 K. PCI5(9) PCI3(g) + Cl₂(g) An equilibrium mixture of the three gases in a 9.30 L container at 530 K contains 0.252 M PCI5, 9.77E-2 M PCI3 and 9.77E-2 M Cl₂- What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 16.6 L? [PC15] = [PC13] = [Cl₂] = M M M CHECK ANSWER

Calculating an equilibrium constant from a heterogeneous equilibrium... 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 amount Fe 2.86 g Н20 2.70 g Fe2O3 2.61 g H₂ 2.34 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 1 C ☐ x10 ☑ 5 ? 18 Ar New Chrome available :

For the chemical equation so, (g) + NO, (g) SO, (g) + NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.31 mol SO, (g) in order to form 1.10 mol SO, (g) at equilibrium. moles of NO, (g): mol

Initial (M) Change (M) Equilibrium (M) -0.00875 0.0209 Consider the reaction of SO2 and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO2(g) + O₂(g) = 2 SO3(g) NEXT > A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂2 at 900 K and allowed to react. At equilibrium, the concentration of SO3 was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 0.00875 re or pull up for additional resources 2.00 1 2SO2(g) 0.0216 2.00 0.0432 0.0148 + 0.0296 2 0.0041 O₂(g) 0.0175 0.0129 11 -0.0175 0.0061 2SO3(g) RESET 0.0350 0.0257

For the generalized chemical reaction A(g) + B(g)  C(g) + D(g) determine whether the concentration of D in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a) concentration of C is increased                              [ Select ]                          ["increase", "decrease", "no change"]            b) concentration of C is decreased                              [ Select ]                          ["increase", "decrease", "no change"]

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"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 1.5 1. flask with 0.88 atm of carbon monoxide gas and 4.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.33 atm of carbon monoxide gas, 3.45 atm of water vapor and 0.55 atm of hydrogen gas. The engineer then adds another 0.22 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm D.P A