We write the relation for Boyle's law in the form, `PV=K_B` when the temperature remains constant. In this relation, the magnitude of `K_B` depends upon the

Options

A. The nature of the gas used in the experiment
B. the molecular mass of gas in the laboratory
C. the atmospheric pressure
D. the quantity of gas enclosed

Answer

To solve the question regarding Boyle's law and the relation \( PV = K_B \), we can follow these steps:

### Step 1: Understand Boyle's Law
Boyle's Law states that for a given mass of gas at constant temperature, the product of pressure (P) and volume (V) is a constant. This can be expressed mathematically as:
\[ PV = K_B \]
where \( K_B \) is a constant for a specific amount of gas at a constant temperature.

### Step 2: Relate to the Ideal Gas Law
The Ideal Gas Law is given by the equation:
\[ PV = nRT \]
where:
- \( P \) = pressure of the gas
- \( V \) = volume of the gas
- \( n \) = number of moles of the gas
- \( R \) = universal gas constant
- \( T \) = absolute temperature

### Step 3: Compare the Two Equations
From Boyle's Law, we have:
\[ PV = K_B \]
From the Ideal Gas Law, at constant temperature, we can rewrite it as:
\[ PV = nRT \]
Since both equations equal \( PV \), we can set them equal to each other:
\[ K_B = nRT \]

### Step 4: Analyze the Dependence of \( K_B \)
In the equation \( K_B = nRT \), we see that \( K_B \) depends on:
- \( n \) (the number of moles of gas)
- \( R \) (the gas constant, which is a constant)
- \( T \) (the absolute temperature, which is constant in this case)

Since \( R \) and \( T \) are constants, the magnitude of \( K_B \) is directly proportional to \( n \), which is the number of moles of the gas.

### Conclusion
Thus, the magnitude of \( K_B \) depends upon the number of moles of the gas, which can also be related to the mass of the gas if the molecular mass is known.

### Final Answer
The magnitude of \( K_B \) depends upon the number of moles of the gas (or the mass of the gas).

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