![For the reaction 3H2(g) + N2(g) =2NH3(8), Keq = 0.297 at 700K. If [H2] = [N2] - [NH3) = 1.62 Mat 700K, which one of the follo](http://img.homeworklib.com/questions/18f063f0-59bf-11eb-a3df-5143233d6e14.png?x-oss-process=image/resize,w_560)
Homework Answers
Calculate the reaction quotient and then compare with equilibrium constant.
![. son- (B) is the correct answer. 312 (9)+ N₂ (g) 21 (g) Keam = 0.297. ( ms] = [Na][]162 M. @ = [NB = (1.627² - [Na] [12]3 (1](http://img.homeworklib.com/questions/19972f70-59bf-11eb-9599-2fe18f609c66.png?x-oss-process=image/resize,w_560)
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For the reaction 3H2(g) + N2(g) =2NH3(8), Keq = 0.297 at 700K. If [H2] = [N2]...
N2(g) + 3H2(g) →2NH3(g) If there is 15.17 g N2 and excess H2 present, the reaction...
N2(g) + 3H2(g) →2NH3(g) If there is 15.17 g N2 and excess H2 present, the reaction yields 14.7 g NH3. Calculate the percent yield for the reaction.
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat...
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
A) For the Haber process, N2(g) + 3H2(g) <---> 2NH3(g), Kp = 4.34 x 10–3 at...
A) For the Haber process, N2(g) + 3H2(g) <---> 2NH3(g), Kp = 4.34 x 10–3 at 300oC. Pure NH3 is placed in a 2.00 L flask and is allowed to reach equilibrium at 300oC. There are 3.00 g NH3 in the equilibrium mixture. Calculate the mass (in g) of H2 in the equilibrium mixture. B) The value of Kc for the reaction is 1.2 . The reaction is started with [H2 ]0 = 0.76 M, [N2]0 = 0.60 M and...
3. Consider the ammonia production reaction, N2(g)+3H2(g) = 2NH3 (g) The equi librium constant for this reaction at 298...
3. Consider the ammonia production reaction, N2(g)+3H2(g) = 2NH3 (g) The equi librium constant for this reaction at 298K is 6.10x 105. When the system starts with 2 mol of NH3 (no H2 or N2), it reaches the equilibrium at the total pressure of 2.0 bar (a) What is the mole fraction of each species at equilibrium? (b) If we increase the total pressure to 3.0 bar, will it be stimulating the decompo- sition of ammonia? Explain
For the reaction 2NH3(g)<->N2(g)+3H2(g), Kc=0.0076 at a particular temperature. If 0.025 M NH3, 0.50M N2, and...
For the reaction 2NH3(g)<->N2(g)+3H2(g), Kc=0.0076 at a particular temperature. If 0.025 M NH3, 0.50M N2, and 0.015 M H2 are mixed in a reaction vessel, is the reaction at equilibrium? If not, in what direction will the reaction shift to reach equilibrium?
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's...
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with O a decrease in the total pressure (T constant) some removal of NH3 from the reaction vessel (V and T constant) an increase in total pressure by the addition of helium gas (V and T constant) a decrease in the total volume of the reaction vessel (T constant) addition of...
Consider the following reaction at equilibrium: (AH° = +92.4kJ) 2NH3(g) = N2(g) + 3H2(0) Le Chateliers...
Consider the following reaction at equilibrium: (AH° = +92.4kJ) 2NH3(g) = N2(g) + 3H2(0) Le Chateliers Principle predicts that the moles of H2(g) in the reaction container will increase with Select one: O a. an increase in the volume of the reaction (constant T) O b. some removal of NH3(g) from the reaction vessel (constant V and T) O c. addition of some N2(g) to the reaction vessel (constant V and T) O d. an increase in total pressure by...
Consider this reaction: 3H2(g) + N2(g) --> 2NH3(g) First, if 5.00 g of H2 is reacted...
Consider this reaction: 3H2(g) + N2(g) --> 2NH3(g) First, if 5.00 g of H2 is reacted with 21.0 g of N2 determine the identity of the limiting reactant. Second, what theoretical mass of product NH3 would be produced?
The ΔHΔH for the reaction N2(g)+3H2(g)N2(g)+3H2(g) →→ 2NH3(g)2NH3(g) is −123.77kJmol−1−123.77kJmol−1 at 1000 K. The heat capacities...
The ΔHΔH for the reaction N2(g)+3H2(g)N2(g)+3H2(g) →→ 2NH3(g)2NH3(g) is −123.77kJmol−1−123.77kJmol−1 at 1000 K. The heat capacities of the reactants and products are CP,m=CP,m= 3.502 RR, 3.466 RR, and 4.217 RR for N2(g)N2(g), H2(g)H2(g), and NH3(g)NH3(g), respectively. Calculate ΔHfΔHf of NH3(g)NH3(g) at 500 KK from this information. Assume that the heat capacities are independent of temperature. Express your answer to four significant figures and include the appropriate units.
Consider the following reaction where K = 0.159 at 723 K: N2(g) + 3H2(g) = 2NH3(g)...
Consider the following reaction where K = 0.159 at 723 K: N2(g) + 3H2(g) = 2NH3(g) A reaction mixture was found to contain 4.65*10*2 moles of N2(g), 3.76x10-2 moles of H2(g) and 5.50*10-4 moles of NH3(g), in a 1.00 Liter container Indicate Truc (T) or False (E) for each of the followingi 1. In order to reach equilibrium NH3(g) must be consumed. 2. In order to reach equilibrium K must decrease. 3. In order to reach equilibrium N, must be...
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
3. Consider the ammonia production reaction, N2(g)+3H2(g) = 2NH3 (g) The equi librium constant for this reaction at 298K is 6.10x 105. When the system starts with 2 mol of NH3 (no H2 or N2), it reaches the equilibrium at the total pressure of 2.0 bar (a) What is the mole fraction of each species at equilibrium? (b) If we increase the total pressure to 3.0 bar, will it be stimulating the decompo- sition of ammonia? Explain
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with O a decrease in the total pressure (T constant) some removal of NH3 from the reaction vessel (V and T constant) an increase in total pressure by the addition of helium gas (V and T constant) a decrease in the total volume of the reaction vessel (T constant) addition of...
Consider the following reaction at equilibrium: (AH° = +92.4kJ) 2NH3(g) = N2(g) + 3H2(0) Le Chateliers Principle predicts that the moles of H2(g) in the reaction container will increase with Select one: O a. an increase in the volume of the reaction (constant T) O b. some removal of NH3(g) from the reaction vessel (constant V and T) O c. addition of some N2(g) to the reaction vessel (constant V and T) O d. an increase in total pressure by...
Consider the following reaction where K = 0.159 at 723 K: N2(g) + 3H2(g) = 2NH3(g) A reaction mixture was found to contain 4.65*10*2 moles of N2(g), 3.76x10-2 moles of H2(g) and 5.50*10-4 moles of NH3(g), in a 1.00 Liter container Indicate Truc (T) or False (E) for each of the followingi 1. In order to reach equilibrium NH3(g) must be consumed. 2. In order to reach equilibrium K must decrease. 3. In order to reach equilibrium N, must be...
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