The rate constant of the elementary reaction 2HI(g) H2(g) +I2(g) is k = 1.97 L mol-1...

The rate constant of the elementary reaction 2HI(g) H2(g) +I2(g) is k = 1.97 L mol-1 s-1 at 604°C, and the reaction has an activation energy of 206 kJ mol-1.

(a) Compute the rate constant of the reaction at a temperature of 767°C. L mol-1 s-1

(b) At a temperature of 604°C, 177 s is required for half of the HI originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 767°C?

Expert Solution

queen_honey_blossom answered 1 year ago

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

For the following reaction: 2HI (g) ----> H2(g) + I2(g), the rate law is rate= k[HI]^2. You are starting with 1.0M HI. How long will the first half-life reaction be? (The professor adds: Note that since you don't know the value for the rate constant k, just leave it in your answers.)

For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an...

For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.057 g H2 and 4.39 g I2. Part A What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.

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

For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25. Starting with 1.00mol of each reactant in a 10.L vessel, how many moles of HI will be present at equilibrium?

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

A student ran the following reaction in the laboratory at 720 K: H2(g) + I2(g) 2HI(g) When she introduced 0.189 moles of H2(g) and 0.218 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.05×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

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

At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g). Calculate the equilibrium constant for the reaction 2H2(g) + 2I2(g) ↔ 4HI(g), 1/2H2(g) + 1/2I2(g) ↔ HI(g), and 2HI(g) ↔ H2(g) + I2(g).

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?

Part A Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Rate law: k[H]^2 k= 6.410^-9 (mols) at 500 K...

Part A Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Rate law: k[H]^2 k= 6.4*10^-9 (mol*s) at 500 K Initial rate = 1.6 * 10^-7 mol (l*s) What will be the concentration of HI after t = 3.65×1010 s ([HI]t) for a reaction starting under this condition? Part B In a study of the decomposition of the compound X via the reaction X(g)⇌Y(g)+Z(g) the following concentration-time data were collected: Time (min) [X](M) 0 0.467 1 0.267 2 0.187 3 0.144 4 0.117 5...

Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.65 L flask at a certain temperature...

Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.65 L flask at a certain temperature initially contains 0.764 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.5 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Kc = ?

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.74 L flask at a certain temperature initially contains 0.767 g H2 and 96.8 g I2. At equilibrium, the flask contains 90.2 g HI.calculate the equillibrium constant (Kc) for the reaction at this temperature. please show work

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.68 L flask at a certain...

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.68 L flask at a certain temperature initially contains 0.767 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.4 g HI. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. Express your answer using two significant figures.

Question