At 1000 °C, for the reaction: 2 H2O(g) ↔ 2 H2(g) + O2(g) Kc = 7.32 x 10-18, what will be the [H2(g)] at equilibrium if 1.00 mol of H2O(g) are placed in a 10.0 L vessel?
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At 1000 °C, for the reaction: 2 H2O(g) ↔ 2 H2(g) + O2(g) Kc = 7.32 x 10-18, what will be the [H2(g)] at equilibrium if 1.00 mol of H2O(g) are placed in a 10.0 L vessel?
1.00 mol Fe(s) and 3.00 mol H2 (g) were placed into a 5.00 L reaction vessel where the Kc for the reaction below is 0.825 at 400K. What is the concentration of hydrogen gas at equilibrium? Fe2O3 (s) + 3H2 (g) <----> 2Fe (s) + 3H2O (g)
The following reaction was carried out in a 3.75 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.50 mol of C, 12.7 mol of H2O, 4.00 mol of CO, and 6.20 mol of H2, what is the reaction quotient Q? Enter the reaction quotient numerically. Q = Consider the reaction CO(g)+NH3(g)⇌HCONH2(g), Kc=0.810 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00...
The equilibrium constant Kc for the following reaction is 8.30. H2(g) + CO2(g) ↔ H2O(g) + CO(g) Initially, 0.40 moles each of H2 and CO2 are injected into a 9.00 L flask. Calculate the concentration of the CO(g) at equilibrium.
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
2 H2O(I) ⇌ 2 H2(g) + O2(g) Le Châtelier's principle predicts that decreasing the volume of the reaction vessel will _______ decreasing the pressure of the reaction vessel a(n) increase in Keq an increase in the concentration of O2 no changes in equilibrium partial pressures a decrease in the concentration of H2 QUESTION 18The slope and intercept of an Arrhenius plot made for the first-order decomposition reaction are -5382.7K and 34.869 at 303K, what is the value of the activation energy (l/mol) at this temperature? QUESTION 19 The rate...
a 10.0 L vessel containing 2.50 x 10-3 mol of H2, 1.00 x 10-3 mol of He, and 3.00 x 10-4 mol of Ne at 35.0oC? what are the partial pressures of each of the gases?
For which reaction will Kp = Kc? C(s) + O2(g) ⇌ CO2(g) 2 H2O(l) ⇌ 2 H2(g) + O2(g) CaCO3(s) ⇌ CaO(s) + CO2(g) H2CO3(s) ⇌ H2O(l) + CO2(g) 2 HgO(s) ⇌ Hg(l) + O2(g)
At 373 K, the following reaction has an equilibrium constant, K = 1.2 x10-2 COCl2 (s) ↔ CO (g) + Cl2 (g) If 1.00 mol of phosgene, COCl2 , is placed in a 10.0 L flask, calculate the concentration of carbon monoxide, CO, at equilibrium.
For the following reaction, 0.500 M of COCl2 is placed in a reaction vessel. Calculate the equilibrium concentrations of all gases at equilibrium. COCl2(g) 2 CO(g) + Cl2(g) Kc = 1.70 x 10-4 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) When 0.256 g of NH3 and 0.480 g if O2 are initially placed in a 1.00 L container at a certain temperature, the N2 concentration at equilibrium is 1.96 x 10 M. Calculate K, for the...
The reaction 2HCL (g) ? H2 (g) +C2 (g) has a kc = 3.2 x 10^-32. A 0.500 -L reaction vessel initially contains 0.025 mol of HCL. A. write an equation for Kc using the chemical entities. B. Set up and complete ICE table. C. Determine the equilibrium concentration of H2 and Cl2