12, mol 12, and 3.24 mol HI, Assuming that the substances are at equilibrium, find the value of K, at 483°C for the reaction of hydrogen and iodine to give hydrogen iodide. The equation is H2 (g) + I2 (9) = 2HI(g) Kc =

Consider the following reaction for which K = 1.60 x 10-7 at some temperature: 2 NOCl (g)  2 NO (g) + Cl2(g)In a given experiment, 0.751 moles of NOCl(g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable "x" in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCl that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration. (Omit units, use 3 sig.fig. and write concentrations less than 1 as 0.###, not as .###. If nothing is present initially, enter 0 for the molarity.)   [NOCl] (M) [NO] (M) [Cl2] (M) Initial       Change       Equilibrium         You have entered that answer before Incorrect. Tries 13/99 Previous Tries   Since K is very small, K = 1.60 x 10-7, very little product will be present at equilibrium, which tells us that very little NOCl will react to reach equilibrium. Because…

Phosphorus pentachloride decomposes according to the chemical equation Kc = 1.80 at 250 °C PC1, (g) PC13 (g) + Cl₂ (g) A 0.1584 mol sample of PC1, (g) is injected into an empty 2.00 L reaction vessel held at 250 °C. Calculate the concentrations of PC1, (g) and PC1₂(g) at equilibrium. [PC1,] = [PC1₂] = 0.0792 Incorrect Incorrect M M

An experimenter places the following concentrations of gases in a closed container: NOB1] = 0.475 M, [NO] = 2.59 x 10-2 M, Bra] = 5.57 x 10-2 M. These gases then react: 2NOB1(g) = 2NO(g) + Br2 (g) At the temperature of the reaction, the equilibrium constant Ke is 3.15 x 10-4. Calculate the reaction quotient, Qe, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. Qc = The concentration of NOBr decreases v

Phosphorus pentachloride decomposes according to the chemical equation Ko PC15 (g) ⇒ PC13 (g) + Cl₂(g) A 0.3476 mol sample of PC15 (g) is injected into an empty 3.95 L reaction vessel held at 250 °C. Calculate the concentrations of PC15 (g) and PC13 (g) at equilibrium. [PCI,] = [PC13] = = 1.80 at 250 °C M M

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures cording to the reaction: PCIs(g) PC13(g) + Cl2(g) At 350°C, 0.675 M PCI s is added to a flask. If Ke=2.50, what are the equilibrium concentrations of each gas?

The equilibrium constant, K., for the following reaction is 5.10×10-6 at 548 K. NH,C(s)NH3(g) + HC(g) Calculate the equilibrium concentration of HCl when 0.501 moles of NH,CI(s) are introduced into a 1.00 L vessel at 548 K. [HCI] = |M

please explain and give complete answer

Consider the following chemical equilibrium: 4 NH, (g) +3 0, (g)=2N, (g) +6 H,Oo (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K_ = I

Consider the following reaction between nitrogen and oxygen and its equilibrium constant at 2000 °C: N2(g) + O2(g) ⇌ 2 NO(g)Kc = 4.10 × 10−4 a)Is the formation of nitrogen monoxide favored at 2000 °C? Explain your answer without doing a calculation. b)What is the nitrogen monoxide concentration when a mixture of 0.40 mol of nitrogen gas and 0.30 mol of oxygen gas reaches equilibrium in a 2.0-L container at 2000°C?