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value: 10.00 points Ch. Ex. 76-cp84-Reaction of Hydrogen with Nitrogen 1 out of 10 attemp Be...
For the reaction represented below, the value of the equilibrium constant, Kp is 3.1 × 10-4 at 700 K. N2 (g) + 3H2 (g) ⇌ 2NH3 (g) Assume that the initial partial pressures of the gases are as follows: P(N2) = 0.411 atm, P(H2) = 0.903 atm, and P(NH3) = 0.224 atm. Which of the following is true? Q < K Q > K Q = K
The value of Kp for the reaction below is is 4.30 × 10–4 at 648 K. 3H2(g)+N2(g)----> 2NH3(g) Part 1) Determine the equilibrium partial pressure of NH3 in a reaction vessel that initially contained 0.900 atm N2 and 0.500 atm H2 at 648 K. _______atm
Ammonia (NH3) is formed via the following reaction between hydrogen (H2) and nitrogen (N2): 3H2(g) + N2(g) 22 NH3(g) For a particular experiment at equilibrium, it was found that the molar concentrations of the three species were as follows: [H2(g)] = 0.162 M, [N2(g)] = 0.100 M. and [NH3(g)] = 0.0100 M. What is the equilibrium constant (K) for this experiment? 4.25 0.617 1.622 0.412 0.235
Nitrogen and hydrogen react to produce ammonia (Haber process). the Kp for the reaction is 4.51 x 10^-5 at 450 degrees C. determine if the following mixtures are at equilibrium at 450 degrees C. If not, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. (Calculate Qp for each case). N2 (g) + 3H2 (g) ⇌ 2 NH3 (g) a) 98 atm Nh3, 45 atm N2, 55 atm H2 b) 57 atm...
1. The simplest ammonia formation is from nitrogen and hydrogen. Consider the reversible reaction N2(g) + 3H2(g) → 2NH3(g) The standard enthaply and Gibbs free energy of formation one mole NH3 is ∆H◦ m = −46.11 kJ mol−1 and ∆G◦ m = −16.78 kJ mol−1 . (a) What is equilibrium constant at standard condition (25°C and 1 atm)? (b) What is equilibrium constant at 60°C and 1 atm? (c) What is the Gibbs free-energy change relative to that under standard...
An evacuated (.e. empty) vessel is charged with 84.9 atm of NH3 (g). The following reaction proceeds to reach equilibrium. 2NH3(g) = N2(g) + 3H2(g) At equilibrium, the partial pressure of H2 remains constant at 64.3 atm. The value of Kp is Report your answer to 3 significant figures. Use scientific notation, i.e. 1.23E4.
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
please show work? Question 38 (8 points) A 50.0 L reaction vessel contains 2.00 mole nitrogen, 3.00 mole hydrogen and 0.500 mole NH3. The mixture is approaching the following equilibrium: N2(g) + 3H2(g) + 2NH3(9) a) Calculate the reaction quotient Q. b) If the value of Kc is 0.500, predict which direction the reaction will go in order to reach equilibrium(to the right, to the left, or no change). Explain your answer.
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 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...