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
the reaction 2HCl=H2(g)+Cl2(g) has a Kc=3.2x10^-32.A 0.500-L reaction vessel initially contains 0.025 mol of HC The reaction 2HCI(g)Hlg) + Cl(e) has a K 0.025 mol of HCI. 3.2x103. A 0.500-L reaction vessel initially contains A. Write an equation for Ke using the chemical entities. B. Set up and complete an ICE table C. Determine the equilibrium concentrations of H2 and Ch. To receive full credit, you must show any appropriate substitutions and all of your algebra work. Use the attached...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A 0.500 L reaction vessel initially contains 0.175 mol of H2S and 6.25×10−2 mol of H2 at 800∘C. Find the equilibrium concentration of [S2].
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 Kc of the reaction H2 (g)+Br2 (g)=2HBr (g) is 2.18×10+6. If the initial concentration of HBr in 12.0L vessel is 3.20 moles, calculate the concentration of H2, Br2 and HBr at equilibrium. Use ICE table. Show calculations and all work & may have to use quadratic equation.
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) +12(g) = 2 HI(g) Kc = 53.3 At this temperature, 0.500 mol H, and 0.500 moll, were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI] =
The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.71 mol H2 and 0.71 mol CO2 are injected into a 5.0−L flask. Calculate the concentration of each species at equilibrium.
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.72 mol H2 and 0.72 mol CO2 are injected into a 4.5−L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H2: M Equilibrium concentration of CO2: M Equilibrium concentration of H2O: M Equilibrium concentration of CO: M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PC13(g) + Cl2(g) = PC15(g) Calculate the equilibrium concentrations of reactant and products when 0.389 moles of PC13 and 0.389 moles of Cl2 are introduced into a 1.00 L vessel at 500 K [PC13] = [Cl] = [PC15] - The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.467 moles of NHACI(S)...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...
-The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.452 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K. [HCl] = _________M -The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g) + I2(g) 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.380 moles of H2and 0.380 moles of I2are introduced into a 1.00...