Consider the equilibrium N2O4(g) ⇌ 2NO2(g). At 500 oC, the equilibrium mixture contained 2.58 M nitrogen dioxide gas.  Calculate the equilibrium concentration of dinitrogen tetroxide if KC at this temperature is 0.726. Provide your answer to two places after the decimal and without units.

Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO,(9) + 0,(9) → 2 SO3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide has the following composition: compound concentration at equilibrium SO2 0.78M O, 1.5M SO3 0.94M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Suppose a 500.mL flask is filled with 1.5mol of CO, 1.1mol of H2O and 1.6mol of H2. The following reaction becomes possible: CO(g)+H2O(g)+CO2(g)+H2(g)   The equilibrium constant K for this reaction is 0.840 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places.

Initial (M) Change (M) Equilibrium (M) 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 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, 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. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)

Nitrogen dioxide decomposes according to the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g)  Where Kp = 4.48 x 10 ^ -13 at a certain temperature. If 0.40 atm of NO is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO (g) and O2 (g)?  P NO =   atm NO P O2 =   atm O2 Use correct significant figures.

Consider the following reaction and associated equilibrium constant at 430 K. 12 (g) + Br2 (g ) ⇌ 2 IBr (g) Kc = 278 If the reaction begins with 0.250 mol of IBr in a 2.00 L flask, calculate the concentration (mol/L) of IBr at equilibrium. Enter your answer with no units. Do not give handwriting solution.

Write the expression for the equilibrium constant K, for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH, as (P NH3)?. If either the numerator or denominator is 1, please enter 1 2 Pb304(s) +→ 6 PbO(s) + O2(g) K =

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 250. mL flask is filled with 1.8 mol of NO3 and 1.1 mol of NO2. The following reaction becomes possible: NO₂(g) + NO(g) + 2NO₂(g) The equilibrium constant K for this reaction is 0.707 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. M × S 1/5

N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =

Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g)+H2O(g)⇌3H2(g)+CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760. °C? Enter your answer with 3 sig figs.