1. Assume that the reaction fort he formation of gaseous hydrogen fluoride (HF) from hydrogen and fluoride has an equilibrium constant of Kc = 1.15x102 at a certain temperature. H2(g) + F2(g) + 2HF(g) In a particular experiment, 3.00 moles of each component were added to a 1.50 L flask. a) Calculate the reaction quotient, Qc, b) Calculate the equilibrium concentrations of all species.

1. Assume that the reaction fort he formation of gaseous hydrogen fluoride (HF) from hydrogen and fluoride has an equilibrium constant of Kc = 1.15x102 at a certain temperature. H2(g) + F2(g) + 2HF(g) In a particular experiment, 3.00 moles of each component were added to a 1.50 L flask. a) Calculate the reaction quotient, Qc, b) Calculate the equilibrium concentrations of all species.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO₂(g) + O₂(g) → 2 SO 3(g) The reaction is exothermic. Suppose a mixture of SO2, O₂ and SO3 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation The temperature is lowered. change in composition The pressure of SO3 will The temperature is raised. The pressure of SO₂ will ? ? î ↑ shift in equilibrium O X to the right to the left (none) to the right to the left (none) S
Consider the following reaction: CO(g) + H₂O(g) = CO₂(g) + H₂(g). Exactly 200 torr each of CO and water vapor were introduced into a 500 ml flask. When the mixture reached equilibrium at 800 K, the partial pressure of CO2 was found to be 99 torr. Calculate the value of Kp.
Suppose 1.000 mol CO and 3.000 mol H2 are putted in a 1.00 L vessel at 1200 k. The equilibrium constant for kc for reverse reaction of CO(g) + 3H2(g) produces CH4(g) + H2O(g) is equals 3.92. find the equilibrium composition of the mixture
Nitrogen and hydrogen react to form ammonia, like this: N,(9)+3H,(g) → 2 NH3(g) The reaction is exothermic. Suppose a mixture of N,, H, and NH, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. olo perturbation change in composition shift in equilibrium Ar to the right The temperature is lowered. to the left The pressure of N2 will (none) to the right to the left The temperature is raised. The pressure of NH3 will v ? go up. (none) go down. not change. ?
The equilibrium constant, Kc, for the following reaction is 1.80×102 at 698 K. 2HI(g) H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [12] = M
calculate the value of the reaction quotient. determine is the system is at equilibrium. if not which direction must the reaction proceed to reach equilibrium
1 A + 2 B → 2 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 8.95 M and [B] is 6.21 M. After the reaction has reached equilibrium,[B] is 1.94 M. Please ignore significant figures for this problem.
A mixture containing 5.6 Atm of N2O and 2.8 Atm of O2 was prepared and after the equilibrium 2 N2O(g) + 3 O2(g) ⇆ 4 NO2(g) was established the O2 partial pressure was found to be 0.31 Atm. What is the equilibrium constant Kp?
Methane and water react to form hydrogen and carbon monoxide, like this: CH₁(9)+H₂O(g) → 3H2(g)+CO(g) The reaction is endothermic. Suppose a mixture of CH 4, H2O, H2 and CO has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium to the right to the left The temperature is raised. The pressure of CH4 will ? ○ (none) to the right to the left The temperature is lowered. The pressure of CO will ? O (none) ×
The formation of ammonia gas from molecular nitrogen and molecular hydrogen gas has the following Kp value. Get the value for the reverse reaction.
Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO,(9)+O2(g) → 2 SO3(g) The reaction is exothermic. Suppose a mixture of SO2, O, and SO, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. dlo perturbation change in composition shift in equilibrium Ar to the right The temperature is lowered. to the left The pressure of SO3 will ? (none) to the right to the left The temperature is raised. The pressure of SO2 will ? O (none)
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