During adiabatic change, specific heat is

Options

A. zero
B. greater than zero but finite
C. less than zero
D. infinite

Answer

To solve the question regarding the specific heat during an adiabatic change, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Adiabatic Process**:
- An adiabatic process is one in which there is no heat exchange with the surroundings. This means that the change in heat (Q) is equal to zero (ΔQ = 0).

2. **Definition of Specific Heat**:
- Specific heat (C) is defined as the amount of heat required to change the temperature of a unit mass of a substance by one degree Celsius (or one Kelvin). The formula for heat transfer can be expressed as:
\[ \Delta Q = nC \Delta T \]
where:
- \( \Delta Q \) = change in heat
- \( n \) = number of moles
- \( C \) = specific heat
- \( \Delta T \) = change in temperature

3. **Applying the Adiabatic Condition**:
- Since we are dealing with an adiabatic process, we know that:
\[ \Delta Q = 0 \]
- Substituting this into the specific heat equation gives us:
\[ 0 = nC \Delta T \]

4. **Analyzing the Equation**:
- For the equation \( 0 = nC \Delta T \) to hold true, either \( n \) (number of moles) or \( \Delta T \) (change in temperature) must be zero. However, in an adiabatic process, we are typically considering a change in temperature, so we focus on the specific heat term.
- Since \( \Delta Q = 0 \), it implies that:
\[ C = \frac{\Delta Q}{n \Delta T} = \frac{0}{n \Delta T} = 0 \]

5. **Conclusion**:
- Therefore, during an adiabatic change, the specific heat (C) is effectively zero.

### Final Answer:
- The specific heat during an adiabatic change is **0**.