1. For the reaction: N2(g)+ 3H2g) 2NH3(g) 4H=-92.4 kJ Complete the Table below by writing: increase,...
The equilibrium constant for the chemical equation N2 g) +3H 2(g) 근 2NH3(g) is Kp = 71.7 at 177 °C. Calculate the value of the Ke for the reaction at 177 °C. Number K,= Tools x 102
Enter your answer in the provided box. For the reaction N2(g) + 3H2(g) = 2NH3(g) K is 8.90 at 337°C. Calculate Kp for the reaction at this temperature.
For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp = 3.50×10−3 at 262 ∘C . What is K for the reaction at this temperature?
Part B? Review | Constants Periodic Table H2NH3 Consider the following reaction: 2NH3(g) = N2(g) + 3H2(g) Submit Previous Answers Correct The equilibrium constant is equal to the concentrations of the products divided by the concentrations of the reactants. The concentrations of both the reactants and the products are raised to a power of the respective coefficient from the balanced chemical reaction. K.= [N] [H] [NH3] Part B What is the numerical value of Kc for the reaction if the...
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...
1. Ammonia synthesis reaction 3H2 (g)+N2 (g) = 2NH3(g) takes place in a reactor under constant temperature 673 K. The initial molar ratio between Hz and N2 is 3:1 (no NH, is present initially), and the reaction is allowed to reach equilibrium. (a) If the pressure is kept constant at 1000 kPa, the molar fraction of NH3 at equilibrium is 0.0385. Please calculate Kp. (b) Using Kp obtained from part (a), please calculate the pressure (still kept constant) of this...
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...
The equilibrium constant expression K p for the reaction 2NH 3 (g) ↔ N2 (g) + 3H2 (g) is __________. A. Kp = PN2(3PH2)3/(2PNH3)2 B. Kp = PNH32/PN2PH23 C. Kp = (2PNH3)2/PN2(3PH2)3 D. Kp = PN2PH23/PNH32
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.
Consider the following reaction: N2(g)+3H2(g)⇌2NH3(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (K) [N2] [H2] [NH3] [Kc] 500 0.115 0.105 0.439 − 575 0.105 M − 0.128 M 9.6 775 0.130 M 0.145 M − 0.0584 Find Kc at 500 K. Find [H2] at 575 K. Find [NH3] at 775 K.