For letter a)
For all of the letters, we need to consider Le Chatelier's principle, which states that any changes made to to the equilibrium, will be opposed by such to get back to equilibrium.
In case hydrogen concentration increases, the equilibrium will try to displace the equilibrium to the reactants, so it will be displaced to the left and more reactants will be produced.
For letter b)
In this case, we have an endothermic reaction, so if the temperature is increased, the reaction will try to absorb that heat, hence, will produce more reactants so that equilibrium may be achieved.
For letter c)
As in this reaction we have the same amount of moles on both sides of the equation (2 and 2), reducing the volume (hence increasing the pressure) will have no effect.
For letter d)
Grinding the pellets only increases the rate of the reaction, it does not affect the equilibrium at all.
Now let us do some Le Chatelier C(s)+H2O (g)←→CO (g) +H2 (g)AH-+131 kJ (in case you...
Please help! Thank you 0.200 An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas) and of the reactants (carbon monoxide and water vapor) in a 1.00-L container. ColgH,o CO,g)+ H How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? Number mol 0.200 An equilibrium mixture contains 0.450 mol of each of...
Is the statement true or false, with respect to the specified reaction in each case?H2(g) + F2(g)<-->2HF(g)If a vessel, containing an equilbrium mixture of these gases, is pressurized by adding helium gas, then the equilibrium position will shift to the right.2SO3(g)<-->2SO2(g) + O2(g)If an equilbrium mixture of these gases is released into a vessel of larger volume, then the equilibrium position will shift to the right.Fe3+(aq) + SCN-(aq)<-->FeSCN2+(aq)If KOH is dissolved in this solution, then the equilibrium position will shift...
For the reaction system: H2 (g) + CO2 (g) → H2O (g) + CO (g) The equilibrium constant is 1.60 at a certain temperature. 1.00 mole each of hydrogen, carbon dioxide is placed in a sealed 5.00 L container. After equilibrium is established, determine the molarity (M) of each species.
Consider the equilibrium CH,(g) + H2O(g) + 206 kJ=CO(g) + 3 H2(g). Which of the following disturbances will NOT cause the system to shift to the right to reestablish equilibrium? Select one: a. The partial pressure of CH4 increases. b. The partial pressure of CO decreases. c. The volume decreases. d. The temperature increases. e. All of these will cause the system to shift to the right
52. A high temperatures carbon monoxide and hydrogen react to produce methanol, CO(g) + 2H2(g) CHOH(g) Δ}":-129 klinol Suppose that in an industrial reactor, the reaction is at equilibrium. For each of the following changes made to the equilibrium system a. The partial pressure of hydrogen is lowered, how will the partial pressures of b. Methanol is rapidly removed from the reactor, how will the pressures of the c· The temperature remains constant while the volume decreases, compressing d. The...
An equilibrium mixture contains 0.550 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g)+H2O(g)−⇀↽−CO2(g)+H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
An equilibrium mixture contains 0.350 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g)+H2O(g)−⇀↽−CO2(g)+H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
(a) Calculate ∆G for the reaction: C(s, graphite) + H2O (g) ↔ CO (g) + H2 (g) where temperature is 700 K, ∆G⁰ = 92 kJ and the initial pressure of each gas is P H2O = 0.67 atm, P CO = 0.23 atm, P H2 = 0.51 atm. (b) What direction would this reaction proceed?
For the reaction: C(s) + H2O(g) CO(g) + H2(g), ΔH° = 131 kJ and ΔS° = 128 J/K at 298 K. At temperatures greater than ______ K, this reaction is spontaneous under standard conditions. a. 1.02 K b. 273 K c. 1023 K d. 753 K
Question 7 (5 points) Consider the equilibrium below: CO(g) + H2O(g) = CO2(g) + H2(g) Kc = 0.0611 at 2000 K If Pco and PH20 are both initially 2.95 atm, what will be the equilibrium partial pressure of H2? Express your answer in decimal format to 3 significant figures. Your Answer: N. Answer Coal, which is primarily carbon, can be converted to natural gas (primarily methane, CH4) by the following exothermic reaction: + C(s) 2H2(g) CH4(g) Which of the following...