Consider the following reaction at 350oC: N2(g) + 3 H2(g) ⇌ 2 NH3(g); Kc=70.
If the concentrations in the reaction mixture at some moment of time are: [NH3] = 0.0100 M, [H2] = 0.0415 M and [N2] = 0.0200M , then
Group of answer choices
the system is at equilibrium and no net change will occur
the system is not at equilibrium and the reaction will proceed to the left
the system is at equilibrium and the reaction will proceed to the left
the system is not at equilibrium and the reaction will proceed to the right
the system is at equilibrium and the reaction will proceed to the right
Consider the following reaction at 350oC: N2(g) + 3 H2(g) ⇌ 2 NH3(g); Kc=70. If the concentrations...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C Part 2. Given the initial conditions below, in which direction is the reaction expected to proceed? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M a neither, the reaction is at equilibrium O b. to the right c. to the left Which of the following acidic solutions has the lowest pH? O a. 0.10 M HMO pka = 8.23 O...
For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105. Use the given concentrations to determine the following. [N2] = 0.0028 M [H2] = 0.0045 M [NH3] = 0.30 M (a) Determine Q at this time. (Omit units.)
The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2 NH3(g) Kc=? Write the equilibrium constant expression (Kc) for this reaction. Calculate the value of Kc at 500. K for the formation of ammonia in part a) using the following measured concentrations for the equilibrium mixture: [N2] = 3.0 x 10-‐2 M; [H2] = 3.7 x 10-‐2 M; [NH3] = 1.6 x 10-‐2 M. [1.7 x 102] Now, calculate the value of Kc for the formation of...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C The value of Kp for this reaction is a. less than ko O b.greater than kc O c equal than ke Consider the reaction: N2 (g)+3 H2 (g)=2 NH3 (g)Kc = 0.0043T = 300 °C Part 1. Given the initial conditions below, which statement is true? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M O a. Q is greater...
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g) b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc c) Calculate the Kp for this reaction d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to nearly 100% completion? Explain f) If Qc...
For the reaction below, Kc = 0.060 at a certain temperature. N2(g) + 3 H2(g) = 2 NH3(g) A flask contains 1.0 M N2, 1.0 M H2, and 1.0 M NH3. Is this system at equilibrium? If not, will the equilibrium concentration of NH3 be greater than, or less than 1.0 M? Justify your answers.
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
A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.61 M, [H2] = 1.26 M, and [NH3] = 0.30 M. Calculate the equilibrium constant, Kc, if the reaction is represented as ( 1 2 ) N2(g) + ( 3 2 ) H2(g) ⇌ NH3(g)
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.
1. For the following reaction N2 (g) + 3 H2(g) — 2 NH3(g) AH° = -92.4 kJ K = 1.245 x 10-5 at 427°C for each change listed, predict the equilibrium shift and the effect on the indicated quantity. Direction of Shift Gt; or no change) Effect on Quantity Change Effect (increase, decrease, or no change) amount of NH3(g) amount of N2(g) (a) decrease in volume (b) Decrease temperature (c) addition of H2(g) (d) addition of NH3(g) (e) removal of...