For the reaction: 2 NO2 (g) + O2 (g) --> 2 NO3 (g) at 923 °C , Kc is 42.5. If 0.0500 moles of NO2 (g), 0.122 moles of O2 (g) and 0.300 moles of NO3 (g) are mixed in a 1.00 liter container at 923 °C, in what direction will the reaction proceed? (Show your calculation to prove that your answer is not a guess.)

Consider the following reaction where Kc = 1.29×10-² at 600 K: ? COCI₂ (9) co (g) + Cl₂ (9) A reaction mixture was found to contain 0.107 moles of COCI₂ (g), 5.31×10-² moles of CO (g), and 3.63×10-² moles of Cl₂ (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: F 1. In order to reach equilibrium COCI₂(g) must be produced. 2. In order to reach equilibrium K must decrease . 3. In order to reach equilibrium CO must be produced. Ⓒ 4. Qc is less than Kc. Ⓒ 5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where Kc = 55.6 at 698 K. H2(g) + I2(g)  ---->  2HI(g) A reaction mixture was found to contain 4.26×10-2 moles of H2(g), 4.04×10-2 moles of I2(g) and 0.270 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals _____   The reaction (fill in the blank) ____ A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.

Part A For the reaction 3H2 (g) + N2 (g) = 2NH3 (g) at 225 °C the equilibrium contant is 1.7 × 102. If the equilibrium mixture contains 0.13 M H2 and 0.018 M N2 , what is the molar concentration of NH3 ? Express your answer to two significant figures and include the appropriate units.

Consider the following reaction where Kc = 1.29×10-2 at 600 K.COCl2(g) CO(g) + Cl2(g)A reaction mixture was found to contain 0.120 moles of COCl2(g), 4.54×10-2 moles of CO(g), and 4.37×10-2 moles of Cl2(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionfill in the blank 2A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.

For the reaction below, the concentrations at equilibrium are [SO₂] = 0.60 M, [O₂] = 0.25 M, and [SO₂] = 1.6 M. What is the value of the equilibrium constant, Ke? 2 SO₂(g) + O₂(g) →→→ 2 SO₂(g) • Report your answer using two significant figures. Provide your answer below:

9) Given the following equilibrium reaction below, indicate which direction the reaction will shift when the indicated stresses are applied (à, ß, or none), AND indicate how the K value will change (increase, decrease or stays same) with the stress. P = 1 atm, unless otherwise specified. ​​CO(g) + Cl2(g) ó COCl2(g) ​ H = –107.6 kJ/mol What will happen if:​​​​​Shift​​​K value i) The pressure is quadrupled​​​​_______​_________________​ ii) The reaction temperature is decreased​​_______​__________________ iii) More COCl2 gas is added​​​​_______​__________________ iv) The volume is doubled​​​​_______​__________________

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C

ook at the reaction below and state which direction the reaction would shift:   You remove mercury(II) oxide, HgO, from the reaction.   2HgO (s) <=> 2Hg (l) + O2 (g) Explain your reasoning

Consider the following reaction where Ke = 1.80 x 10-4 at 298 K. NH4HS(s) ⇒ NH3 (9) + H₂S(9) A reaction mixture was found to contain 0.0584 moles of NH4HS(s), 0.00833 moles of NH3(g), and 0.0134 moles of H₂S(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium.