Consider the following reactions: A ⇌ B, K₁=7.60 A ⇌ C, K₂=2.00 What is K for the reaction C ⇌ B?

For the equilibrium reaction: 2NO2 ⇌ N2O4 When 0.2 mol of NO2 is added to a 1.0 L flask at 25°C. K = 2.6. What are the equilibrium concentrations?

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g)   1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms   2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown.   3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown.   4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.

will the stress causes the equilibrium to shift towards reactants or products, or will it have no effect? 1. PCl5 ⇌ PCl3+Cl2     ΔH>0     (stress:Increase Volume) 2. Co(H2O)2+6(aq) +4Cl-(aq) ⇌ CoCl2-4(aq) +6H20    ΔH>0    (stress:Decrease temperature) 3. N2 + 3H2 ⇌ 2NH3(g)   ΔH<0    (stress: increase pressure by adding helium)

Consider a hypothetical chemical reaction: A(g) ⇌ 3B(g) You put 1.00 mol of gas B in a 50.0 L container, seal it and wait for the reaction to reach equilibrium. At equilibrium you find 0.25 mol of gas A in the container. What is the K value for this reaction?

When K is less than zero, the reactants are favored and the reaction proceeds in the reverse direction. True False

For the reaction 2CO2 (g) ⇌ 2CO (g) + O2 (g), Kc = 6.4 x 10-7. If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

2SO2 (g) + O2 (g) ⇌ 2SO3 (g) Predict the direction of the shift if SO2 is added to the equilibrium reaction mixture.