The value of universal gas constant R depends on :

Options

A. temperature of gas
B. volume of gas
C. number of moles of gas
D. units of volume and pressure

Explanation

To determine what the value of the universal gas constant \( R \) depends on, we can analyze the ideal gas law and the units involved. Here’s a step-by-step solution:

### Step 1: Understand 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
- \( T \) = temperature of the gas

### Step 2: Rearranging the Ideal Gas Law
From the ideal gas law, we can express \( R \) as:
\[ R = \frac{PV}{nT} \]
This equation shows that \( R \) is derived from the values of pressure, volume, number of moles, and temperature.

### Step 3: Analyzing the Units
The value of \( R \) can vary depending on the units used for pressure, volume, and temperature. Common values of \( R \) include:
- \( R = 8.314 \, \text{J/(mol·K)} \) (SI units)
- \( R = 0.0821 \, \text{L·atm/(mol·K)} \) (atmospheric pressure)
- \( R = 8.314 \, \text{L·kPa/(mol·K)} \) (kilopascals)

### Step 4: Conclusion on Dependence
The value of the universal gas constant \( R \) depends on the units of pressure and volume used in the calculations. It does not depend on the actual values of pressure, volume, number of moles, or temperature, but rather on the units in which these quantities are expressed.

### Final Answer
The value of the universal gas constant \( R \) depends on the units of volume and pressure.

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