sopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H7OH(g) ⇌ C2H6CO(g) + H2(g) At 180°C, the equilibrium constant for the decomposition is 0.45. If 37 mL (d = 0.785 g/mL) of isopropyl alcohol is placed in a 6.5 L vessel and heated to 180°C, what percentage remains undissociated at equilibrium?

A chemist places 1.00 mol of each hydrogen and carbon dioxide in a 1.25-L container at 800oC. This reaction occurs:H2(g) + CO2(g) ⇌ H2O(g) + CO(g)When equilibrium is reached, 0.49 mol of gaseous carbon monoxide is in the container. Based on this information, what is the value of the equilibrium constant, K?

Consider the following reaction between nitrogen and oxygen and its equilibrium constant at 2000 °C: N2(g) + O2(g) ⇌ 2 NO(g)Kc = 4.10 × 10−4 a)Is the formation of nitrogen monoxide favored at 2000 °C? Explain your answer without doing a calculation. b)What is the nitrogen monoxide concentration when a mixture of 0.40 mol of nitrogen gas and 0.30 mol of oxygen gas reaches equilibrium in a 2.0-L container at 2000°C?

Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H7OH(g) ⇌ C2H6CO(g) + H2(g) At 180°C, the equilibrium constant for the decomposition is 0.45. If 45 mL (d = 0.785 g/mL) of isopropyl alcohol is placed in a 3.5 L vessel and heated to 180°C, what percentage remains undissociated at equilibrium? ______. %

Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.23-L flask at a certain temperature initially contains 27.3 g CO and 2.33 g H2. At equilibrium, the flask contains 8.63 g CH3OH. Part ACalculate the equilibrium constant  (Kc)   for the reaction at this temperature.

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq) + CH3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH,CO₂ 1.01 M O↑ increase CH3NH2 1.22 M O decrease O↑ increase O decrease O (no change) O (no change) A CH,CO, 0.64 M O↑ increase O decrease O (no change) CH, NH3 1.04 M O ↑ increase O decrease O (no change) HCH CO₂ 0.33 M O↑ increase O decrease O(no change) CHÍNH, 0.50 M O↑ increase O decrease O (no change) B CH,CO, 1.01 M O increase O decrease O (no…

Water gas is a 1:1 mixture of carbon monoxide and hydrogen gas and is called water gas because it is formed from steam and hot carbon in the following reaction: H2 O(g) + C(s) ⇌ H2(g) + CO(g). Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and hydrogen at high temperature and pressure in the presence of a suitable catalyst.(a) Write the expression for the equilibrium constant (Kc) for the reversible reaction2H2(g) + CO(g) ⇌ CH3 OH(g)                                ΔH = −90.2 kJ(b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added?(c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed?(d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added?(e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased?(f) What will happen to the concentrations of H2, CO,…

A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH,NH,(aq) → CH;CO,(aq)+CH,NH,(2q) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.6. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound expected change in cor concentration concentration vessel HCH,CO, 0.96 M O T increase OI decrease O (no change) CH, NH, 0.88 M O f increase OI decrease O (no change) A CH,Co, 0.54 M O f increase OI decrease O (no change) CH,NH, 0.45 M O f increase OI decrease O (no change) HCH, CO, 0.88 M f increase OI decrease O (no change) CH,NH, 0.77 M O f increase OI decrease O (no change) B CH, Co, 1.09 M O increase OI…

The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.0×10^-3. If the equilibrium mixture contains [NO2] = 0.055 M , what is the molar concentration of N2O4?