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 7 × 106 at a certain temperature. In an experiment, 6.70 × 10-² mole of NO, 1.00 × 10 ³3 mole of Cl2, and 6.80 moles of NOCI are mixed in a 2.10–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 left. The reaction is at equilibrium. The reaction will proceed to the right.

Calculating an equilibrium constant from a partial equilibrium composition Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 2.0 L flask with 4.4 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 2.0 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = р x10 Ś ? olo 18 Ar B

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

Consider the chemical reaction system represented by the following equation: 2 SO2 (g)  + O2 (g)  ⇆   2 SO3 (g)  The initial concentrations were 0.40 M SO2 (g) 1.6 M O2 (g) and 29.7 M 2 SO3 (g).  The equilibrium concentration of SO2 is 1.2 M.  Determine the value of Keq.

At a certain temperature, Kc = 6.0 x 10^-4 for the reaction between sulfur trioxide gas and gaseous hydrogen fluoride to produce gaseous sulfur hexafluoride and water vapour: SO3(g) + 6HF(g) = SF6(g) + 3H20(g) Calculate the equilibrium concentration of sulfur hexafluoride that would result if 1.8 mol of sulfur trioxide was mixed with 5.6 mol of hydrogen fluoride in a 2.1 L container.

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.

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

At 454 K, Al,Cl6(g) reacts to form Al;Cl,(g) according to the equation 3 Al,Cl,(g) = 2 Al;Cl,(g) In an experiment at this temperature, the equilibrium par- tial pressure of Al,Cl(g) is 1.00 atm and the equilibrium partial pressure of Al;Cl,(g) is 1.02 × 10-2 atm. Compute the equilibrium constant of the preceding reaction at 454 K.

A student ran the following reaction in the laboratory at 282 K: 2CH2C12(g)=CH4(g)+ CCI4(g) When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =

For the reaction 2NO(g) + O2(g) → 2NO2(g) at a certain temperature, the equilibrium concentrations were found to be [NO2] = 5.7 × 10–3 M, [O2]= 1.0 × 10–2 M, and [NO] = 2.0 × 10–3 M. Calculate the value of the equilibrium constant from these data.