The question you uploaded is asking to find the volume of oxygen gas at 37°C when its volume is 10 L at 27°C, with the assumption of constant pressure and constant number of moles of gas.

To solve this, we can use Charles' Law, which states that the volume of a gas is directly proportional to its temperature when the pressure and the number of moles are constant. The formula for Charles' Law is:

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

Where:

• $V_1$ and $V_2$ are the initial and final volumes.
• $T_1$ and $T_2$ are the initial and final temperatures in Kelvin.

Given:

• $V_1 = 10 \, \text{L}$
• $T_1 = 27^\circ C = 27 + 273 = 300 \, \text{K}$
• $T_2 = 37^\circ C = 37 + 273 = 310 \, \text{K}$

Now, solve for $V_2$ (the final volume):

$V_2 = V_1 \times \frac{T_2}{T_1} = 10 \times \frac{310}{300}$

Let's calculate that. Given values V1 = 10 # Initial volume in liters T1 = 300 # Initial temperature in Kelvin (27°C) T2 = 310 # Final temperature in Kelvin (37°C)

Calculate the final volume using Charles' Law

V2 = V1 * (T2 / T1) V2The final volume of the gas at 37°C is approximately 10.33 L.

Thus, the correct answer is 10.33 L.

Would you like any further explanation or have additional questions on this topic?

Here are some related questions you might find helpful:

1. How does temperature affect the volume of a gas under constant pressure?
2. What is the relationship between temperature and volume in gas laws?
3. What would happen to the volume if the temperature was reduced instead?
4. How do you convert Celsius to Kelvin when using gas laws?
5. What is the ideal gas law and how does it compare to Charles' Law?

Tip: Always remember to convert temperatures to Kelvin when using gas laws to avoid errors in calculation!