For the reaction A(g)+2B(g)--><--- C9g) 2 moles of A and 3 moles of B are placed in a 6.00 Liter container. At equilibrium, the concentration of A is .300mol/L. What is the concentration of B at equilibrium and what is the value of K?
For the reaction A(g)+2B(g)--><--- C9g) 2 moles of A and 3 moles of B are placed...
For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container. A(g) + 2B(g) C(g) At equilibrium, the concentration of A is 0.210 mol/L. What is the value of K?
2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05. What is the equilibrium constants Kc and Kp for the reaction 4NH3 + 2N2(g) + 6H2(g)? Kp = 400 Kc = 7.62 x 10 3. For the reaction given below, 10.00 moles of A and 25.00 moles of B are placed in a 5.00-L container at 120 °C. A(g) +2B(g) → C(g) At equilibrium, the concentration of A is 0.5 mol/L. What is the...
2. (Type III) The reaction N2(g) + 3H2(g) → 2 NH3(g) starts with 6.00 moles of N2 and 6.00 moles of H2 in a 4.00L flask. a. What are the concentrations of N2 and H2 initially? b. If, at equilibrium, the concentration of N2 is 1.14 M. what are the concentrations of H2 and NH3 at equilibrium? c. What is the value of equilibrium constant K?
When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.107 M. A student ran the following reaction in the laboratory at 297 K: 2NO(g)+ Br2(g)2NOBr(g) When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.107 M. Calculate the equilibrium constant, Kc, she obtained for this reaction....
2.000 moles of A and 0.800 moles of B are sealed in a 5.000 L container at At 425.0 K. When equilibrium is reached, the concentration of D in the container is 0.3470 M. Determine the value of the equilibrium constant Kcfor the reaction at this temperature. 2 A (g) + 2 B (s) ⇄ C (g) + 2 D (g)
For the reaction: N_2(g) + O_2(g) 2NO(g) If 0.200 moles of NO gas is placed in theta 2.00 L container at 800K, what will be the equilibrium concentrations.
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u IIULS reaction: CÓ (g) + 3 H (g) + CH4 (g) + H2O (G) 1. At 25°C, Keq=4.0. What must be the Co] at equilibrium If the equilibrium concentrations of [H.]= 2.0M. (CH) = 5.0M, and (HO) = 3.OM? Answer: 0.469 M The ICE table is a way to keep track of what is happening in the reaction vessel. The initial concentrations if given...
Consider the following reaction: 2 HI(g) H2(g) + I2(g) If 2.29 moles of HI, 0.309 moles of H2, and 0.363 moles of I2 are at equilibrium in a 17.8 L container at 774 K, the value of the equilibrium constant, Kp, is
A mixture of 9.22 moles of A, 10.11 moles of B, and 27.83 moles of C is placed in a one-liter container at a certain temperature. The reaction is allowed to reach equilibrium. At equilibrium the number of moles of B is 18.32. Calculate the equilibrium constant for the reaction:  A (g) + 2 B (g)<-> 3 C (g) Answer is supposed to be .0832. How? Also, how do you determine which way the reaction is going? Thanks
A student ran the following reaction in the laboratory at 686 K: H2(g) + I2(g) 2HI(g) When she introduced 0.200 moles of H2(g) and 0.230 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.18×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?