At a high enough temperature, the equilibrium constant is 4.00 for the gas-phase isotope exchange reaction; H2 + D2 ⇀↽ 2 HD Calculate the equilibrium partial pressures if 0.50 atm of H2 and 0.10 atm of D2 were initially present in a 20.0-L system at 488 K. What is the extent of reaction at equilibrium?

At a high enough temperature, the equilibrium constant is 4.00 for the gas-phase isotope exchange reaction; H2 + D2 ⇀↽ 2 HD Calculate the equilibrium partial pressures if 0.50 atm of H2 and 0.10 atm of D2 were initially present in a 20.0-L system at 488 K. What is the extent of reaction at equilibrium?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 15P

See similar textbooks

Similar questions

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .
Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g) 6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?
For the following combustion reactions, predict whether compression will favour the formation of products or reactants, or whether there will be no change in the equilibrium composition:(a) C4H8(g) + 6 O2(g) → 4 CO2(g) + 4 H2O(I)(b) C2H5OH(I) + 3(1)/(2) O2(g) → 2 CO2(g) + 3 H2O(I)(c) C6H12O11(s) + 3(1)/(2) O2(g) → 6 CO2(g) + 6 H2O(I)(d) 2 C6H5NH2(1) + 17(1)/(2) O2(g) → 12 CO2(g) + 7 H2O(I) +2 NO2(g)
Explain the effect of each of the following stresses on the position of the equilibrium SO;(g) 2 SO02(g) + 2 O2(g) The reaction as written is endothermic. (a) O2(g) is added to the equilibrium mixture without changing volume or temperature. (b) The mixture is compressed at constant temperature. (c) The equilibrium mixture is cooled. (d) An inert gas is pumped into the equilibrium mixture while the total gas pressure and the temperature are kept constant. (e) An inert gas is added to the equilibrium mixture with- out changing the volume.
The equilibrium constant for the reaction H,S(g) + I(g) 2 2 HI(g) + S(s) at 110°C is equal to 0.0023. Calculate the reaction quo- tient Q for each of the following conditions and determine whether solid sulfur is consumed or produced as the reac- tion comes to equilibrium. (a) P, = 0.461 atm; Pµ;s = 0.050 atm; PHI (b) P, = 0.0 atm 0.461 atm; R1,s = 0.050 atm; PHI = 9.0 atm
The equilibrium constant for the reaction H2(g) + I½(s) = 2 HI(g) at 25°C is K = 0.345. (a) If the partial pressure of hydrogen is P1, = 1.00 atm and solid iodine is present, what is the equilibrium partial pressure of hydrogen iodide, PH1, at 25°C? (b) An excess of solid I, is added to a container filled with hydrogen at 25°C and a pressure of 4.00 atm. Calcu- late the pressures of H2(g) and HI(g) reached at equilibrium.
A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous NO was present. Assume that the reaction SO-(9) + NO2 (g) = SO; (g) + NO(9) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K =
For the above reaction, if the value of Kp (expressed in terms of the partial pressures in atm) was 16.6 at 857°C, what would be the value of Keg (expressed in terms of the molar concentrations) at 857°C? (No units required.)
15 16 17 18 19 20 21 22 23 24 25 Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(9) 3 NO,(g)+H,O(1) At a certain temperature, a chemist finds that a 5.3 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 23.3 g NO 18.5 g NO2 14.4 g H,0 182.7 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = | Submit Ass Continue MacBook Air 26
(b) The equilibrium constant for the reaction H2 + 12 2HI at 700°C is 55. Calculate the equilibrium concentration of the reactants & products, when the initial concentration ofI, & 1 are 2.55 moles/dm3 each.