O Macmillan Learning A 4.20 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseo concentration of B steadily increased until it reached 1.20 M, where it remained constant. A(s) B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remair

Given the equilibrium equation: 3A + Be = 2C2 If 2.50 moles of A and 0.500 moles of B are added to a 2.00 L container, an equilibrium is established in which the [C] is found to be 0.250 M. a) Find [A] and [B] at equilibrium. Answer b) Calculate the value of the equilibrium constant Keq

1C. Please don't write on a paper. I can't understand handwritten.

3. Please don't write on a paper. I can't understand handwritten.

4. help use sig figs pls

For the following reaction, Kcis 144 at 200°C. If 0.400 mol of both A and B are placed in a 2.00-liter container at that temperature, what will be the concentration of C at equilibrium? A (g) + B (g) = C (g)

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N, (g) + 2H,0(g)=2 NO(g) + 2H, (g) K,=2. × 10-9 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 1.9 atm of water vapor. Use this data to answer the questions in the table below. yes Can you predict the equilibrium pressure of H2, using only the tools x10 available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit.

1) State the equilibrium expression/equation for the provided reaction: A + 3 B) f C + 3D(3) [K2] (8) 2) 2.44 mol of gaseous hydrogen bromide is added to an empty 3.16 L container. When values

A mixture initially contains A A , B B , and C C in the following concentrations: [A] [A]A_1 = 0.400 M M , [B] [B]B_1 = 1.10 M M , and [C] [C]C_1 = 0.700 M M . The following reaction occurs and equilibrium is established: A+2B⇌C A+2B⇌C At equilibrium, [A] [A]A_2 = 0.290 M M and [C] [C]C_2 = 0.810 M M . Calculate the value of the equilibrium constant, Kc

(Incorrect) For the reaction 2A(g) = B(g) + C(g) at 700 °C, Kc = 3.92×104. Calculate the number of moles of B present at equilibrium if 3.49 moles of A is heated to 700 °C in a 8.48-L container. 0.00784 mol (Your answer) 0.396 mol 3.36 mol 9.24×104 mol 0.0665 mol (Correct answer)