Chemistry
posted by David .
The decomposition of IBr(g)into I2 (g) and Br2 (g) is first order in IBr with k = 0.00255/sec.
(a)Starting with [IBr] = 1.50M, what will [IBr] become after 2.50 minutes?
(b)How long, in minutes, will it take for [IBr] to go from 0.500M to 0.100M?
(c)What is the halflife for this reaction in seconds?
(d)Enough IBr is added to an evacuated container to make [IBr] = 0.350M. How long will it take [I2] = 0.100M?
Respond to this Question
Similar Questions

Chemistry
The decomposition of IBr(g)into I2 (g) and Br2 (g) is first order in IBr with k = 0.00255/sec. (a)Starting with [IBr] = 1.50M, what will [IBr] become after 2.50 minutes? 
Chemistry
The decomposition of IBr(g)into I2 (g) and Br2 (g) is first order in IBr with k = 0.00255/sec. (a)Starting with [IBr] = 1.50M, what will [IBr] become after 2.50 minutes? 
ChemistryDrBob222
Arrows disappeared from below added them back to the equations. The decomposition of IBr(g)into I2 (g) and Br2 (g) is first order in IBr with k = 0.00255/sec. (a)Starting with [IBr] = 1.50M, what will [IBr] become after 2.50 minutes? 
ChemistryDrBob222
Arrows disappeared from below added them back to the equations. ? 
ChemistryDrBob222
Arrows disappeared from below added them back to the equations. ? 
AP CHEMISTRY
For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.590 mol IBr in a 2.50L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2? 
chem
For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.570 mol IBr in a 2.50L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2? 
Chemistry
A sealed 1.0L flask is charged with .500mol I2 and .500mol Br2 and an equilibrium reaction esues: I2(g)+Br2(g)=2IBr(g) When the container contents achieve equilibrium, the flask contains .84 mol of IBr. What is the value of the eqilibrium … 
chemistry
At a certain temperature, Keq is 4.13 x 10^5 for the equilibrium: 2IBr(g) ↔ I2(g) + Br2(g) Assume that the equilibrium is established at the above temperature by adding only the reactant to the reaction flask. What are the concentrations … 
chemistry
Consider the following reaction in the solvent CCl4 in a 1L flask: 2IBr(g)<>Br2(g)+I2(g) What is the equilibrium moles of IBr, Br2 and I2 are 0.2, 0.1 and 0.1, calculate the equilibrium constant Kc.