The following reaction is investigated (assume an ideal gas mixture): 2N20(g) + N2H4(g) 3N2(g) + 2H2O(g) Initially there are 0.100 mol of N20 and 0.25 mol of N2H4, in a 10.O-L container. If there are 0.059 mol of N20 at equilibrium, how many moles of N2 are present at equilibrium? O 4.1 x 10^-2 1.2 x 10^-1 6.2 x 10^-2 O 2.1 x 10^-2 none of these

= 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

An equilibrium mixture contains 0.2500.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.2000.200 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)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 0.3000.300 mol once equilibrium has been reestablished? moles of CO2CO2 =

[References] chemist placed a mixture of CO, (g) and CF,(9) into a flask at a particular temperature. These gases react: CO2 (g) + CF (g) 2COF2 (g) Iter this mixture came to equilibrium, she found that it contained 0.42 mole fraction of CF4 and 0.16 mole fraction of COF2. Calculate K, at this temperature for this reaction.