Two identical cylinders contains helium at 1.5 atm and argon at 1 atm respectively. If both the gases are filled in one of the cylinder, the pressure would be

Options

A. 1 atm
B. 1.75 atm
C. 2.5 atm
D. 0.5 atm

Answer

To solve the problem of finding the total pressure when helium and argon are combined in one cylinder, we can follow these steps:

### Step 1: Understand the Given Information
We have two identical cylinders:
- Cylinder 1 contains helium at a pressure of 1.5 atm.
- Cylinder 2 contains argon at a pressure of 1 atm.

### Step 2: Combine the Gases
When both gases are combined in one cylinder, we need to find the total pressure exerted by the mixture of helium and argon.

### Step 3: Use Dalton's Law of Partial Pressures
According to Dalton's Law of Partial Pressures, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each gas. Therefore, we can express the total pressure (P_total) as:

\[ P_{\text{total}} = P_{\text{He}} + P_{\text{Ar}} \]

Where:
- \( P_{\text{He}} \) is the pressure of helium (1.5 atm).
- \( P_{\text{Ar}} \) is the pressure of argon (1 atm).

### Step 4: Calculate the Total Pressure
Now, substituting the values into the equation:

\[ P_{\text{total}} = 1.5 \, \text{atm} + 1 \, \text{atm} \]
\[ P_{\text{total}} = 2.5 \, \text{atm} \]

### Step 5: Conclusion
The total pressure when both gases are filled in one cylinder is 2.5 atm.

**Final Answer:** The total pressure is 2.5 atm.

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