The average rate of reaction: H2 (g) + I2 (g) → 2HI is 0.001 M/sec. Initial...

Question

Question

The average rate of reaction: H2 (g) + I2 (g) → 2HI is 0.001 M/sec. Initial [HI] was 0. 2 M. What is [HI] 1.5 min?

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

The average rate of reaction: H2 (g) + I2 (g) → 2HI is 0.001 M/sec. How...

The average rate of reaction: H2 (g) + I2 (g) → 2HI is 0.001 M/sec. How will be the concentration of product changed after 1.5 min?
The rate constant for the gaseous reaction H2(g) + I2(g) → 2HI(g) is 2.42 × 10−2/(M·s)...

The rate constant for the gaseous reaction H2(g) + I2(g) → 2HI(g) is 2.42 × 10−2/(M·s) at 400°C. Initially an equimolar sample of H2 and I2 is placed in a vessel at 400°C and the total pressure is 1690 mmHg. (a) What is the initial rate (M·min) of formation of HI? (__________) (b) What are the rate of formation of HI and the concentration of HI (in molarity) after 13.4 min? Rate of formation = (_______) (c) [HI] = (_______)...
Consider the reaction: H2(g) + I2(s) = 2HI (g) Given an initial mass of 19.02g H2 an...

Consider the reaction: H2(g) + I2(s) = 2HI (g) Given an initial mass of 19.02g H2 an excess of I2 and assuming that all of the reactant is conserved to products and non is lost calculate the mass (g) of HI produced by the reaction?

Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the...

Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 5.92×1010 s ([HI]t) for a reaction starting under the condition in the simulation?
Given that the reaction H2 (g) + I2 (g) <--> 2HI (g) is at equilibrium and...

Given that the reaction H2 (g) + I2 (g) <--> 2HI (g) is at equilibrium and the measured concentrations of each component of the reaction are [H2] = 0.22 M, [I2] = 0.22 M, and [HI] = 1.56 M, write the equilibrium expression and then calculate Keq.
H2(g) + I2(s) → 2HI(g) Given an initial mass of 15.28 g H2, an excess of...

H2(g) + I2(s) → 2HI(g) Given an initial mass of 15.28 g H2, an excess of I2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction.

H2(g)+I2(g)=2HI(g) The value of Kp for the reaction is 61.0 at 905 °C. What is the...

H2(g)+I2(g)=2HI(g) The value of Kp for the reaction is 61.0 at 905 °C. What is the equilibrium partial pressure of HI in a sealed reaction vessel at 905 °C if the initial partial pressures of H2 and I2 are both 0.260 atm and initially there is no HI present?
For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration...

For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration of HI (g) at equilibrium if the initial concentration of each substance is 0.0600 M and the reaction mixture is allowed to come to equilibrium. (Hint: ICE Table)
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....

The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...

Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a...

Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.02, 0.021 and 0.160 M respectively. The value of Keq for this reaction is __________.