Calculate Keq for the reaction below given the following information: initial partial pressure of the reactant is 1.47 torr and the equilibrium partial pressure of carbon dioxide is 0.283 torr. This gaseous reaction is reversible and at equilibrium. H2CO3(g) double arrows H2O (g) + CO2 (g) 5.19 0.0545 0.238 0.0675 0.0457

give handwritten

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.

= O KINETICS AND EQUILIBRIUM Using Le Chatelier's Principle to predict the result of changing... Acetylene and oxygen react to form carbon dioxide and water, like this: 2C₂H₂(g) +50₂(g) → 4CO₂ (g)+2H₂O(g) Suppose a mixture of C₂H₂, O₂, CO₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some H₂O is removed. Some C₂H, is added. change in composition The pressure of C₂H₂ will The pressure of O₂ will The pressure of O₂ will The pressure of CO₂ will ? ? ? ? ? V go up. go down. not change. shift in equilibrium O to the right to the left x O (none) 3/5 to the right to the left (none)

The reaction below was allowed to react at 375 degrees Celcius until it formed an equilibrium. At equilibrium, the 16.2 L container was found to contain 1.9 mol SiF4, 1.1 mol H2O, 3.5 mol SiO2, and 2.9 mol HF. What is the Kc of the reaction at this temperature?  SiF4 (g) + 2H2O (g) <--> SiO2 (s) + 4HF(g)

For the reversible decomposition reaction of dinitrogen pentaoxide (0.308 atm) to yield nitrogen dioxide (0.211 atm) and oxygen (0.076 atm), what is the value for the equilibrium constant, K?  The equilibrium pressures for each chemical are provided in parentheses after their name.  This reaction occurs in the gas phase.      629     0.0110     0.00159     0.0521     19.2

For the reaction: COCI2 (g) + CO + Cl2 (g) (g) At 100°C the reaction has an equilibrium constant of 2.2 x 10-10, If 1.00 mole of phosgene (COCI2) is placed in a 10.0 L flask, calculate the concentration of carbon monoxide at equilibrium. Write your answer in standard form (not scientific notation).

2. Please don't write on a paper. I can't understand handwritten.

Record your two digit answer. Use the following information to answer the next 4 questions. An equilibrium system was established in a 1.00 L flask at a certain temperature as represented by the following equation ICI(g) + Cl₂(g) ICI,(g) + energy brown yellow-green bright yellow At equilibrium the flask contained 0.0571 mol of ICI(g), 1.07 mol of Cl₂(g), 1.87 mol of ICl3(g) The value of the equilibrium constant for this system is 30.6 Record your 3-digit answer Under these conditions, the equilibrium system in Question 20 favours the forward the reverse neither reaction. ?

= KINETICS AND EQUILIBRIUM Setting up a reaction table Suppose a 500. mL flask is filled with 1.7 mol of N₂ and 0.10 mol of NH3. This reaction becomes possible: N₂(g) + 3H₂(g)2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N₂. You can leave out the M symbol for molarity. initial change equilibrium N₂ 0 0 H₂ 0 0 0 NH3 0 0 00 1/5 X