Part A A 55.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.30 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂(g) in the reactor? Express your answer in atmospheres to two significant figures. VE ΑΣΦ P(CO₂) = Submit Request Answer Part B What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. [5] ΑΣΦ m = ? ? g 04 atm

The equilibrium constant, Kc, for the following reaction is 1.25 at 659 K. 2NH3 (9) N2(g) + 3H₂(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 659 K, the equilibrium concentration of H₂(g) is found to be 0.609 M. Calculate the concentration of NH3 in the equilibrium mixture. [NH3] = Submit Answer Use the References to access important values if needed for this question. M Submit Answer Retry Entire Group 8 more group attempts remaining [Review Topics] [References] Use the References to access important values if needed for this question A student ran the following reaction in the laboratory at 679 K: H₂(g) + I₂(g) → 2HI(g) When she introduced 0.208 moles of H₂(g) and 0.237 moles of I2 (g) into a 1.00 liter container, she found the equilibrium concentration of I2 (g) to be 0.0625 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = | Retry Entire Group 8 more group attempts remaining'

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.

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.

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

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204(g) = 2NO2(g) A 1.000-L flask is charged with 0.0300 mol of N204. At equilibrium, 0.0204 mol of N204 remains. Calculate the Kc for this reaction. (Enter only the numerical value to three significant figures without units.) Answer:

Show work..don't give Handwritten answer....don't use Ai for answering this

5. Consider the equilibrium where Kc = 85.0 at 460°C. The following mixture was prepared in a reactor at 460 °C with the concentrations [SO2] = 0.0200 M; [NO2] = 0.0200 M; [NO] = 0.100 M; [SO3] = 0.100 M. What will the concentrations of the four gases be when equilibrium is reached? SO2 (g) + NO2 (g) - NO (g) + S03 (g); Ke = 85.0 I 0.02 O. 02 C -x E 6.02- 0,02-0 0.ltx 0.lto 一× +x 十 LNOJ CSOPJ ) T02=x)co-02-) కంటె CN6 kc

Consider the following reaction at equilibrium. 4CuO (s) + CH4 (8) CO₂ (g) + 4Cu (s) + 2H₂O(g) AH = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of H₂O(g) can be decreased by removing Cu adding CH4 decreasing the reaction temperature decreasing the reactor volume adding an inert gas