# A #4 L# container holds #19 # mol and #20 # mol of gasses A and B, respectively. Groups of four of molecules of gas B bind to three molecule of gas A and the reaction changes the temperature from #210^oK# to #120^oK#. How much does the pressure change?

The pressure drops from 168 atm to 22.2 atm.

I'll respond to a query from another Wisconsinite!

Determining the change in the number of moles from the reaction is the most challenging aspect of this problem.

Please

If we assume that gasses A and B are ideal, we have all the information we need to calculate the initial pressure. (In reality, this is not the case at 120K!)

The problem indicates that the reaction proceeds as follows: The two types of gases react to form a new gas C.

Since we only have roughly 5% more B than A prior to the reaction, we know that gas B is the limiting reagent in this case. We will assume that the reaction proceeds to completion in order to eliminate gas B after the reaction.

Please

Due to the stoichiometry of the reaction

We can compute the pressure following the reaction, assuming once more that the ideal gas law is true.

By signing up, you agree to our Terms of Service and Privacy Policy

To calculate the pressure change, we can use the ideal gas law, (PV = nRT).

- First, we need to find the initial and final pressures.
- Then, we can find the difference to determine the pressure change.

Given:

- Initial temperature ((T_i)) = 210 K
- Final temperature ((T_f)) = 120 K
- Initial moles of gas A ((n_A)) = 19 mol
- Initial moles of gas B ((n_B)) = 20 mol
- Initial volume ((V)) = 4 L

Using the ideal gas law: [P_i = \frac{n_A RT_i}{V} + \frac{n_B RT_i}{V}] [P_f = \frac{n_A RT_f}{V} + \frac{n_B RT_f}{V}]

[P_i = \frac{19 \times R \times 210}{4} + \frac{20 \times R \times 210}{4}] [P_f = \frac{19 \times R \times 120}{4} + \frac{20 \times R \times 120}{4}]

Calculate (P_i) and (P_f).

Then, find the pressure change: [∆P = P_f - P_i]

By signing up, you agree to our Terms of Service and Privacy Policy

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

- If i run down some stairs and stop, what happens to your kinetic energy and your initial gravitational potential energy?
- What is the Clapeyron equation?
- A #7 L# container holds #12 # mol and #18 # mol of gasses A and B, respectively. Every three of molecules of gas B bind to one molecule of gas A and the reaction changes the temperature from #350^oK# to #175 ^oK#. By how much does the pressure change?
- Is pressure caused by the collision of gas molecules with their surroundings?
- Is Stefan Boltzmann law related to global warming?

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7