The equilibrium constant Kc for the reaction below is 0.00384 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0257 M and [Br] = 0.0888 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant Kc for the reaction below is 0.00384 at a certain temperature. Br2(g) ⇌...
At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 × 10−3. If the initial concentrations are [Br2] = 0.0480 M and [Br] = 0.0470 M, calculate the concentrations of these two species at equilibrium. [Br2]eq = ___M [Br]eq = ____M
Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 × 10−3. If the initial concentrations are [Br2] = 0.0390 M and [Br] = 0.0370 M, calculate the concentrations of these two species at equilibrium. [Br2]eq [Br]eq
The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362 M, calculate the [Br] = The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362 M, calculate the [Br] =
For the reaction, Br2(g) ⇌ 2Br(g) the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C. Determine the initial and equilibrium concentrations of Br if the initial and equilibrium concentrations of Br2 are 5.90 × 10−3 M and 5.20 × 10−3 M, respectively. [Br]i = M [Br]e = M
For the reaction, Br2(g) = 2Br(g) the equilibrium constant, Kis 1.10 X 10 at 1280°C. Determine the initial and equilibrium concentrations of Brif the initial and equilibrium concentrations of Br are 5.80 x 10-3 Mand 5.10 x 10 3 M, respectively. [Br]:- [Br] - M
For the following reaction, the equilibrium constant Kc is 0.60 at a certain temperature. If the concentration of NO(g) and NOBr(g) are both 0.10 M, at equilibrium, what is the concentration of Br2(g)? 2NO(g) + Br2(g) ⇌ 2NOBr(g)
1-The equilibrium constant Kc for the equation 2H2(g) + CO(g) ⇌ CH3OH(g) is 11 at a certain temperature. If there are 2.63 × 10−2 moles of H2 and 7.15 × 10−3 moles of CH3OH at equilibrium in a 6.29−L flask, what is the concentration of CO? ?M 2-In an analysis of the following reaction at 100°C,Br2(g) + Cl2(g) ⇌ 2BrCl(g) the equilibrium concentrations of the reactants were found to be [Br2] = 4.0×10−3M and [Cl2] = 7.7 ×10−3M. The equilibrium...
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 18.1−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] =___ M Br2] = ___M [HBr] = ____M
At a certain temperature, the equilibrium constant, Kc , is 0.00401 for the reaction Cl2(g)−⇀↽−2Cl(g) A. If 3.05 g Cl2Cl2 is placed in a 3.00 L flask at this temperature, what are the equilibrium concentrations of Cl2 and Cl? B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 4.50 L while the temperature is held constant. What are the new equilibrium concentrations of Cl2 and Cl? C. Following the establishment of...
Equilibrium and ICE Table 1) The equilibrium constant (KC) at 1280 °C for the following reaction is 1.1 x 10-3. What are the equilibrium concentrations for Br2(g) and Br(g) if the initial concentration of Br2 is 0.125 M? Br2(g) ⇌ 2 Br(g) 2) Consider the reaction for the decomposition of H2S at 800 °C where the KC is 1.67 x 10-7. In a 0.5 L reaction vessel the initial concentration of H2S is 0.0125 mol at 800 °C. What are...