Question

A certain reaction is first order in H2 and first order in I2. Use this information...

A certain reaction is first order in H2 and first order in I2. Use this information to complete the table below. Round each of your answers to 3 significant digits..

[H2] [I2] Initial Rate of Reaction

0.949M. 1.59M. 3.00 X 10^3 M/s

0.949. 0.694 ?

2.03 0.742 ?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order...
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI and the rate constant is 9.7×10−6M−1s−1. If the initial concentration of HI is 0.100 M . What is its molarity after a reaction time of 5.00 days?
At a certain temperature the rate of this reaction is first order in HI with a...
At a certain temperature the rate of this reaction is first order in HI with a rate constant of :0.0632s 2HIg=H2g+I2g Suppose a vessel contains HI at a concentration of 1.28M . Calculate how long it takes for the concentration of HI to decrease to 17.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.63 L flask at a certain...
Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.63 L flask at a certain temperature initially contains 0.767 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.6 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Express your answer using two significant figures.
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order...
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI and the rate constant is 9.7×10^−6 M^−1s^−1. If the initial concentration of HI is 0.130 M... What is its molarity after a reaction time of 7.00 days? What is the time (in days) when the HI concentration reaches a value of 7.5×10^−2 M ?
For the reaction H2 + I2 (g)2HI (g) with Kc = 54.3 at 698 K, if...
For the reaction H2 + I2 (g)2HI (g) with Kc = 54.3 at 698 K, if the initial amounts were 0.800 mole H2 and 0.500 mole I2 in a 5.25-L vessel at 698 K, write the ICE table, and what will be the amounts of reactants and products (in mole(s)) when equilibrium is attained?
Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following...
Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M . Find [H2] at 340 ∘C . Express your answer using two significant figures. (Please show me the step-by-step math needed to achieve this answer, that is what I'm having trouble with, thank you!) T(∘C) [H2] [I2] [HI] [Kc] 25 0.0355 0.0388 0.922 − 340 − 4.50×10−2 M 0.391 M 90.6 445 4.85×10−2 M...
The equilibrium constant Kc for the reaction below is 82.3 at a certain temperature. H2(g) +...
The equilibrium constant Kc for the reaction below is 82.3 at a certain temperature. H2(g) + I2(g) double arrows 2HI (g) If you start with .355 M of hydrogen iodide, what will the concentrations of HI, H2, I2 be at equilbrium?
Some measurements of the initial rate of a certain reaction are given in the table below....
Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 1.08M 1.38M 0.720/Ms 1.08M 1.93M 1.41/Ms 3.76M 1.38M 8.73/Ms Use this information to write a rate law for this reaction, and calculate the value of the rate constant k.Be sure your value for the rate constant has the correct number of significant digits. Also be sure your answer has the correct unit symbol.
Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following...
Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T(∘C) [H2] [I2] [HI] [Kc] 25 0.0355 0.0388 0.922 − 340 − 4.50×10−2 M 0.394 M 9.6 445 4.90×10−2 M 4.76×10−2 M − 50.2 Find [H2] at 340 ∘C. Find [HI] at 445 ∘C.
The initial concentrations of I2 and I− in the reaction below are each 0.0401 M. If...
The initial concentrations of I2 and I− in the reaction below are each 0.0401 M. If the initial concentration of I−3 is 0 M and the equilibrium constant is Kc=0.25 under certain conditions, what is the equilibrium concentration (in molarity) of I−? I−3(aq)↽−−⇀I2(aq)+I−(aq) Your answer should include two significant figures.