Using the Kf and Kb equations with electrolytes A certain liquid X has a normal boiling point of 110.90 °C and a boiling point elevation constant K=1.66 °C-kg mol -1 .A solution is prepared by dissolving some ammonium sulfate ((NH SO,) in 150. g of X. This solution boils at 112.2 °C. Calculate the mass of (NH) SO, that was dissolved. Round your answer to 2 significant digits. Explanation Check

Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g) + O2(g) + H2 (g) = ;N¿H4(g)+NO2(g), : ? by making use of the following information: 1. N2 (g) + O2 (g): = 2NO(g), K1 4.10 x 10-31 2. N2 (g) + 2H2 (g) = - N2H4(g), K2 7.40 x 10–26 3. 2NO(g) + O2 (g) = 2NO2(g), K3 = 6.00 x 10-13 Express your answer numerically. • View Available Hint(s) Vo AEO ? Kgoal =

While ethanol (CH3CH2OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH2CH2) with water vapor at elevated temperatures.  A chemical engineer studying this reaction fills a 500. mL flask with 4.6atm of ethylene gas and 4.2atm of water vapor. When the mixture has come to equilibrium he determines that it contains 2.7atm of ethylene gas and 2.3atm of water vapor.  The engineer then adds another 1.5atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.

Select the reaction for which K, = Kc. 2 CO, (g) + 2 CF,(g) =4 COF, (g) NH,NO, (s) = N,O(g) + 2H,O(g) 2 H, S(g) + SO, (g) = 3 S(s) + 2 H,O(g) O 2 Na, O, (s) + 2CO,(g) =2 Na,CO;(s) + 0,(g)

CS2 (g) + 4 H2 (g) <====> CH4 (g) + 2 H2S (g)   Calculate the value of Keq if the equilibrium concentrations are [CS2] = 0.140, [H2] = 0.250, [CH4] = 0.0200, and [H2S] = 0.0400.

Only typed sollution.

At 25 °C and 765 Torr, carbon dioxide has a solubility of 0.0342 M in water. What is its solubility at 25 °C and 1410 Tor? M S =

Suppose that 8.00 mol of both O2 and N₂O gases are introduced into a 4.00 L closed flask. When the system comes to equilibrium, 3.00 mol of nitrogen monoxide (NO) gas has formed, shown below. Determine the equilibrium concentrations of all entities in the flask. 2 N₂O(g) + O₂ (g) = = 4 NO(g) UPLOAD A FULL SOLUTION WITH AN ICE TABLE, CALCULATIONS, AND FINAL ANSWERS WITH UNITS AND THE CORRECT NUMBER OF SIGNIFCANT DIGITS.

The answer is already given which is 0.173 mol H2  I'd like to know the complete solution. Thanks!

Consider the equilibrium at 25 °C 2 SO3(g)  <==> 2 SO2(g) + O2(g)          Kc= 3.58 x10-3 Suppose that 0.15 mol SO3(g), 0.01 mol SO2(g), and 0.0075 mol O2(g) are placed into a 10.0 L flask at 25 °C. Which of the following statements is true? Q > Kcand will shift from right to left.   Q < Kc and  will shift from right to left.   Q > Kcand will shift from left to right.   Q = Kcand the system is at equilibrium.   Q < Kc and  will shift from left to right.