Consider the following equilibrium: 2NH3(g) mc018-1.jpg N2(g) + 3H2(g); DH = 92 kJ What change should be made in order to increase the value of Kp for this reaction
A. Increase the pressure. |
B. Decrease the temperature. |
C. Increase the temperature. |
D. Decrease the pressure. |
E. Nothing; Kp cannot be changed. |
2NH3(g) -----> N2(g) + 3H2(g); dH = 92 kJ
the above reaction is an endo thermic reaction.
if you increase the temperature then the reactnts react together well and in creases the pressure of products sothat the value of Kp increases.
Answer: C
Kp = (PN2) * (PH2)^3 / (PNH3)^2
Consider the following equilibrium: 2NH3(g) mc018-1.jpg N2(g) + 3H2(g); DH = 92 kJ What change should...
N2(g) + 3H2(g) = 2NH3(g) AH° = .92 kJ Select the conditions under which the yield of ammonia is the highest. High temperature and high pressure High temperature and low pressure Low temperature and high pressure Low temperature and low pressure
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 Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g) What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
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 this reaction: N2(g) + 3H2(g) <==> 2NH3(g) If the Kc for the reaction is 4.5 x 10^4 at 127 degrees celsius, what is the equilibrium constant, Kp at the same temperature?
Consider the following equilibrium N2(g) +3H2(g) 2NH3(g) ΔG--34. kJ Now suppose a reaction vessel is filled with 8.06 atm of nitrogen (N2) and 6.48 atm of ammonia (NH3) at 176. °C. Answer the following questions about this system: rise fall Under these conditions, will the pressure of N2 tend to rise or fall? Dio Is it possible to reverse this tendency by adding H? In other words, if you said the pressure of N2 will tend to rise, can that...
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 equilibrium: N2(g) + 3H2 (g) = 2NH3(g) AG°= - 34. kJ Now suppose a reaction vessel is filled with 2.01 atm of nitrogen (N) and 5.74 atm of ammonia (NH) at 812. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH2 tend to rise or fall? fall Is it possible to reverse this tendency by adding H,? x 6 ? yes In other words, if you said the pressure...
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a. Is this reaction spontaneous? Explain. b. Predict the sign of AS. Explain. C. Based on your answer to part b, is this reaction exothermic or endothermic? Explain. For the reaction N2(g) + 3H2(g) 2NH3 (8) a. Using values in Appendix Cin your book, calculate AHⓇ and AS. b. Assuming that AHºand ASº don't change with temperature, calculate the value for AG at 400K Is...
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...