May I get some help on this please, thank you very much. ### Educational Exercise: Gas Volume Calculation**Question 2:**If \( k_2 = 0.97 \) atm·L, what would be the volume (in liters) of a gas at 586 mmHg?**Question 3:**Consider the following: *Note:* There is additional context required for Question 3, but it is not provided in the image. For Question 2, to solve for the volume of gas given the pressure, you can use the following steps and the principle of Boyle's Law (assuming the temperature and amount of gas remain constant). Boyle's Law can be expressed as:\[ P_1 V_1 = P_2 V_2 \]Where:- \( P \) is the pressure- \( V \) is the volumeGiven:- \( k_2 = P_1 V_1 = 0.97 \) atm·L- \( P_2 = 586 \) mmHg (convert this to atm: 586 mmHg * (1 atm / 760 mmHg) ≈ 0.77 atm)By applying the known values to Boyle's Law:\[ 0.97 \text{ atm·L} = 0.77 \text{ atm} \times V_2 \]Therefore, solving for \( V_2 \):\[ V_2 = \frac{0.97 \text{ atm·L}}{0.77 \text{ atm}} ≈ 1.26 \text{ L} \]So, the volume \( V_2 \) would be approximately 1.26 liters.**Note:** It's essential to have the complete context for Question 3 to further elaborate on it.

Given: K = 0.94 atm. L = 714.4 mmHg. L (Since: 1 atm = 760 mmHg ) The given pressure = 586…

Answered: 2. If k, = 0.97 atm-L, what would be…

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2. If k, = 0.97 atm-L, what would be the volume (in liters) of a gas at 586 mmHg?

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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May I get some help on this please, thank you very much.

### Educational Exercise: Gas Volume Calculation

**Question 2:**
If \( k_2 = 0.97 \) atm·L, what would be the volume (in liters) of a gas at 586 mmHg?

**Question 3:**
Consider the following:

*Note:* There is additional context required for Question 3, but it is not provided in the image.

For Question 2, to solve for the volume of gas given the pressure, you can use the following steps and the principle of Boyle's Law (assuming the temperature and amount of gas remain constant). Boyle's Law can be expressed as:

\[ P_1 V_1 = P_2 V_2 \]

Where:
- \( P \) is the pressure
- \( V \) is the volume

Given:
- \( k_2 = P_1 V_1 = 0.97 \) atm·L
- \( P_2 = 586 \) mmHg (convert this to atm: 586 mmHg * (1 atm / 760 mmHg) ≈ 0.77 atm)

By applying the known values to Boyle's Law:

\[ 0.97 \text{ atm·L} = 0.77 \text{ atm} \times V_2 \]

Therefore, solving for \( V_2 \):

\[ V_2 = \frac{0.97 \text{ atm·L}}{0.77 \text{ atm}} ≈ 1.26 \text{ L} \]

So, the volume \( V_2 \) would be approximately 1.26 liters.

**Note:** It's essential to have the complete context for Question 3 to further elaborate on it.

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