Use the reaction below to complete the table by answering with (1) shift to reactants, (2) shift to products, or (3) no effect. CO(g) + 2H2(g)  CH3OH(l); H is endothermic Equilibrium Effected by a:                                    Reaction will ___________. Pressure of CO is increased Remove a portion of CH3OH Pressure is decreased due to a volume increase Reaction is cooled Hydrogen gas is selectively removed

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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature.  If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?

A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant.   A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont

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Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by      (1) removing O2(g)?      (2) adding N,(g)?      (3) adding water?      (4) expanding the container at constant pressure?      (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?

Dry ice (solid carbon dioxide) is placed in a sealed container. It sublimes to produce carbon dioxide gas and reaches equilibrium at a given temperature. If the amount of dry ice in the container is doubled, then _____________.  (After choosing the correct answer justify why in your own words why you chose that answer)                                                                                       CO2 (s) = CO2 (g) A)The amount of CO2 (g) would double.  B)The amount of CO2 (g) would increase but not double. C)The amount of CO2 (g) would not change.  D)The equilibrium amount of CO2 (s) would be less.

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Type the word True or False in the provided space for the following. Consider the following system at equilibrium where Kc = 9.52x10-2 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CCl4 (g) → 2 CH₂Cl₂ (g) The production of CH₂Cl2 (g) is favored by: decreasing the temperature. increasing the pressure. increasing the volume. removing CH₂Cl2. removing CCl4. I. II. III.____ IV. V.

Consider the following equilibrium: 2NO₂(g) → N₂O4 (g) AG = -5.4 kJ Now suppose a reaction vessel is filled with 0.202 atm of nitrogen dioxide (NO₂) at 504. °C. A Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O needed to reverse it. V Round your answer to 2 significant digits. Orise fall O yes no atm 0