Homework Answers
Adding product will shift the reaction in the direction of reactant as per Le chatelier Principle
So, Equilibrium moves to reactant side
SO, concentration of NH3 will increase and that of H2 will decrease
Value of Kc will not change because temperature is constant.
Answer: option 2
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Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H)...
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...
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: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ...
Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ Le Châtelier's principle predicts that a decrease in temperature will decrease the value of the equilibrium constant O increase the value of the equilibrium constant decrease the partial pressure of CO increase the partial pressure of CO2 (g) decrease the partial pressure of O2 (g) Consider the following reaction at equilibrium: 2NH3 (g) = N2 (g) + 3H2(g) AH° = +92.4 kJ Le Châtelier's...
Consider the following equilibrium 2NH3 (g)N2(g)+3H, Now suppose a reaction vessel is filled with 2.89 atm...
Consider the following equilibrium 2NH3 (g)N2(g)+3H, Now suppose a reaction vessel is filled with 2.89 atm of amoia (NH3) and 2.79 atm of nitrogen (N2) at 944. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N2 tend to rise or fall? fall Is it possible to reverse this tendency by adding H2? In other words, if you said the pesure of N2 will tend to rise, can that be changed to a...
1) The reaction below is exothermic 2SO2 (g) + O2(g) = 2803(g) + heat Le Châtelier's...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
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.
Question 39 2 pts Which of the following changes is most likely to decrease the reaction...
Question 39 2 pts Which of the following changes is most likely to decrease the reaction rate for the chemical reaction? 2CO(g) + O2(g) → 2CO2(g) O adding a catalyst to the reaction mixture adding twice as much O2 to the reaction mixture O removing some CO from the reaction mixture tripling the temperature of the reaction mixture Question 40 2 pts If two aqueous solutions with concentrations of 0.3 M sugar and 0.5 M sugar respectively are separated by...
Consider the following equilibrium: 2NH3(g)=N2(g)+3H2(g) delta G^o=34 kJ Now suppose a reaction vessel is filled...
Consider the following equilibrium: 2NH3(g)=N2(g)+3H2(g) delta G^o=34 kJ Now suppose a reaction vessel is filled with 0.311 atm of ammonia NH3 and 1.45 atm of nitrogen N2 at 1093 °C. Answer the following questions about this system: Under these conditions will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H2? In other words, if you said the pressure of NOH3 will tend to rise, can that be changed to...
The equilibrium constant, Kc, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g)...
The equilibrium constant, Kc, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 15.7 L container at 723K contains 0.284 mol of NH3(g) and 0.437 mol of N2, the equilibrium concentration of H2 is__________ M.
Consider the chemical reaction 2NH3(g) ó N2(g) + 3H2(g). The equilibrium is to be established in...
Consider the chemical reaction 2NH3(g) ó N2(g) + 3H2(g). The equilibrium is to be established in a 50.0 L container at 1,000 K, where Kc = 4.0 × 10-2. Initially, 6.10 x 105 moles of NH3(g) are present. Calculate the amount of H2 presentat equilibrium. [H2] =_____
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...
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: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ Le Châtelier's principle predicts that a decrease in temperature will decrease the value of the equilibrium constant O increase the value of the equilibrium constant decrease the partial pressure of CO increase the partial pressure of CO2 (g) decrease the partial pressure of O2 (g) Consider the following reaction at equilibrium: 2NH3 (g) = N2 (g) + 3H2(g) AH° = +92.4 kJ Le Châtelier's...
Consider the following equilibrium 2NH3 (g)N2(g)+3H, Now suppose a reaction vessel is filled with 2.89 atm of amoia (NH3) and 2.79 atm of nitrogen (N2) at 944. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N2 tend to rise or fall? fall Is it possible to reverse this tendency by adding H2? In other words, if you said the pesure of N2 will tend to rise, can that be changed to a...
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.
Question 39 2 pts Which of the following changes is most likely to decrease the reaction rate for the chemical reaction? 2CO(g) + O2(g) → 2CO2(g) O adding a catalyst to the reaction mixture adding twice as much O2 to the reaction mixture O removing some CO from the reaction mixture tripling the temperature of the reaction mixture Question 40 2 pts If two aqueous solutions with concentrations of 0.3 M sugar and 0.5 M sugar respectively are separated by...
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