Response:
Here's my calculation
Clarification:
Assume the starting concentrations of H₂ and I₂ are 0.030 and 0.015 mol·L⁻¹, respectively.
We need to determine the initial concentration of HI.
1. We will need a chemical equation with concentrations, so let's compile all the information in one location.
H₂ + I₂ ⇌ 2HI
I/mol·L⁻¹: 0.30 0.15 x
2. Calculate the concentration of HI
3. Plot the initial values
The graph below visualizes the initial concentrations as plotted on the vertical axis.
Response: The rate constant at 525 K is,
Rationale:
Based on the Arrhenius equation,
or,
where,
= rate constant when
=
= rate constant when
=?
= activation energy for the process =
R = gas constant = 8.314 J/mole.K
= initial temperature = 701 K
= final temperature = 525 K
Substituting the provided values into this formula yields:
Thus, the rate constant at 525 K is,
Answer: The mole fraction of nitrogen is calculated to be 0.4615.
Explanation: In the mixture of nitrogen () and hydrogen (
), the mole ratio established is 1: 1.5.
At this juncture, we identify that () serves as the limiting reagent.
When 0.4 moles of () are produced, it will require 0.4 moles of (
) along with 3.4 moles of (
).
The total amount of remaining () ends up being 0.6, while the amount of (
) left in the mixture is 0.3 moles.
The mole fraction of () is computed as 0.6 divided by the sum of 0.6, 0.4, and 0.3, resulting in 0.4615.