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A glucose (C6H12O6) solution is prepared by dissolving [x] g glucose in [y] g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?  Report your answer with the correct number of significant figures and the correct units.

Consider the following reaction:  Xe(g) + 2 F 2(g) → XeF 4(g) A reaction mixture initially contains [x] M Xe and [y] M F 2. If the equilibrium concentration of XeF4 is [z] M, find the equilibrium constant (K c) for the reaction.   Report your answer with the correct number of significant figures.

At a certain temperature the equilibrium constant,  K c, equals [w] for the reaction: 2 ICl( g) ⇌ I 2( g) + Cl 2( g). What is the equilibrium concentration of ICl if [y] mol I 2 and [y] mol Cl 2 are placed in a 2.00 L evacuated flask?   Report your answer with the correct number of significant figures and the correct units.

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO 2( g) + O 2( g) ⇌ 2 SO 3( g). If the concentrations are [SO 2] = 1.20 M, [O 2] = 0.45 M, and [SO 3] = 1.80 M, calculate Q and determine which is statement is true for the system.

The following reaction is exothermic. What set of conditions will always lead to the equilibrium shifting to the left? 2 NO(g) + Br2(g) ⇌ 2 NOBr(g)

What is the reducing agent in the redox reaction represented by the following cell notation? Zn(s) ∣ Zn2+(aq) ‖ Ag+(aq) ∣ Ag(s)

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system?CO2(g) + 2 H2O(l) ⇌ CH4(g) + 2 O2(g)ΔH° = +890 kJ

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Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 102 A reaction mixture contains 0.35 M I 2, 0.31 M Br 2 and 3.5 M IBr. Calculate Q and determine which of the following statements is TRUE concerning this system?