Consider the gas phase reaction H2 + I2 = 2HI at equilibrium at T= 870 K...

Consider the gas phase reaction H2 + I2 = 2HI at equilibrium at T= 870 K and p = 1 bar. If ∆G˚ (870K, 1 bar) = - 48.96 kJ, determine K, ξ and the equilibrium amounts of H2, I2 and HI (in mol) if the intial composition was n˚(H2) = 0.300 mol, n˚(I2) = 0.400 mol, and n˚(HI) = 0.200 mol

Expert Solution

queen_honey_blossom answered 1 year ago

The gas phase reaction H2 + I2 --> 2HI is second order. Its rate constant at...

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For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25....

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H2 + I2 yields 2HI At the start of the reaction 1 mole of I2 and 1 mole of H2 are put into a 10 liter container. There is no HI present. At the reaction temperature Keq is 64 What is the equilibrium concentrations for H2, I2 and HI?

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Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture at equilibrium contains pressures of H2 = 0.958 atm, I2 = 0.877 atm, and HI = 0.020 atm. At the same temperature, a second reaction mixture (not at equilibrium) contains pressures of H2 = 0.621 atm, I2 = 0.621 atm, and HI = 0.101 atm. What will be the partial pressure of HI when the second reaction mixture reaches equilibrium? a) 0.0144 atm b)...

At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g)....

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At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature,...

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?

A student ran the following reaction in the laboratory at 720 K: H2(g) + I2(g) 2HI(g)...

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For the following reaction: 2HI (g) ----> H2(g) + I2(g), the rate law is rate= k[HI]^2....

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