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202 solutions

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Q. Find the equilibrium concentrations of A, B, and C for a=1, b=1, and c=2. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas.

Solved • Feb 14, 2020

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Q. For the reaction at 700°C, Kc = 0.534. Calculate the number of mole of H2 that are present at equilibrium if a mixture of 0.200 mole of CO and 0.200 mole of H2O is heated to 700°C in a 30.0 L container.

Solved • Feb 13, 2020

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Q. The equilibrium constant Kc for the reaction below is 83.3 at a certain temperature. H2(g) + I2(g) <-> 2HI(g). If you start with 0.325 M hydrogen iodide, what will the concentrations of H2, i2, and HI be at equilibrium?

Solved • Feb 13, 2020

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Q. The equilibrium constant, Kp, for the following reaction is 0.215 at 523 K: PCl5(g) ⇌ PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.01 atm at 523 K.

Solved • Feb 11, 2020

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Q. The equilibrium constant, Kc, for the following reaction is 1.80x10^-2 at 698 K. 2HI(g) ⇌ H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.235 moles of HI are introduced into a 1.00 L vessel at 698 K.

Solved • Feb 11, 2020

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Q. A student ran the following reaction in the laboratory at 665 K: H2(g) + I2(g) ⇌ 2HI(g) When she introduced 0.212 moles of H2(g) and 0.232 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of HI(g) to be 0.352 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

Solved • Feb 11, 2020

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Q. The equilibrium constant, Kc, for the following reaction is 1.90x10^-3 at 244 K. 2NOBr(g) ⇌ 2NO(g) + Br2(g) When a sufficiently large sample of NOBr(g) is introduced into an evacuated vessel at 244 K, the equilibrium concentration of Br2(g) is found to be 0.177 M. Calculate the concentration of NOBr in the equilibrium mixture.

Solved • Feb 11, 2020