Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + Cl2(g) = 2NOCI(g) is 3 x 10° at a certain temperature. In an experiment, 5.50 × 10¬2 mole of NO, 3.00 × 103 mole of Cl2, and 2.70 moles of NOCI are mixed in a 3.10–L flask. What is Q, for the experiment? x 10 (Enter your answer in scientific notation.) In which direction will the system proceed to reach equilibrium? The reaction will proceed to the right. The reaction is at equilibrium. The reaction will proceed to the left.

The equilibrium constant, K, for the following reaction is 1.29x10-2 at 600 K. COC,(g) CO(g) + Cl2(g) + C2(g) Calculate the equilibrium concentrations of reactant and products when 0.262 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI,] = [CO] [Ch] MMM

Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)

The following reaction has an equilibrium constant, Kc equal to 3.59 at 900 °C. CH4(g) + 2H₂S(g) — CS2(g) + 4 H2(g) At a particular time during the reaction, the following composition has been found: [CH4(g)] = 1.20 M, [CS2(g)] = 1.15 M, [H₂S(g)] = 1.31 M, [H2(g)] = 1.85. Predict the activity of the reaction during the particular time above. The reaction should go to the left (or reverse) The reaction should go to the right (or forward) The reaction is at a standstill The reaction activity cannot be determined There is no basis for prediction.

The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] =  M [PCl3] =  M [Cl2] =  M

The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.

N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)

The equilibrium constant, K, for the following reaction is 9.52×10 2 at 350 K. CH, (g) + CCI, (g)=2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.310 moles of CH, and 0.310 moles of CCI, are introduced into a 1.00 L vessel at 350 K. [CH ] M [CCL] =D M [CH,Cl, ] = M

The equilibrium constant K₁, K2 and K3 for the reactions below are S(s) + O₂(g) → SO₂(g), K₁ = 4.2 × 1052 2S (s) +30₂(g)2SO3(g), K₂ = x 2SO2(g) + O2(g)2SO3(g), The value of K₂ is 9.8 × 1028 2.6 × 1075 □ 6.7 × 10¹2 1.34 × 1032 9.8 x 10128 K3= 5.6 x 1023

A chemical engineer is studying the following reaction: CH₂(g) + 2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³. р The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound CH4 H₂S CS₂ H₂ CHA H₂S CS₂ H₂ pressure 5.65 atm 3.56 atm 5.77 atm 7.93 atm 4.69 atm 1.62 atm 6.73 atm 11.81 atm OO expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase olo ↓decrease ↓decrease ↓ decrease ↓decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no change) (no…