Heat change of a process, in which volume remains constant, is represented by

Options

A. `Delta U`
B. `Delta H`
C. `Delta G`
D. `Delta n`

Answer

To solve the question regarding the heat change of a process in which the volume remains constant, we can follow these steps:

### Step 1: Understand the First Law of Thermodynamics
The first law of thermodynamics states that the change in internal energy (ΔU) of a system is equal to the heat added to the system (Q) minus the work done by the system (W):
\[ \Delta U = Q - W \]

**Hint:** Recall that the first law of thermodynamics relates heat, work, and internal energy.

### Step 2: Identify Work Done at Constant Volume
In a thermodynamic process, work done (W) can be expressed as:
\[ W = -P \Delta V \]
where P is the pressure and ΔV is the change in volume.

Since the volume remains constant in this process, ΔV = 0. Therefore, the work done is:
\[ W = -P \cdot 0 = 0 \]

**Hint:** Remember that if there is no change in volume, there is no work done by the system.

### Step 3: Substitute Work Done into the First Law Equation
Substituting W = 0 into the first law equation gives:
\[ \Delta U = Q - 0 \]
Thus, we can simplify this to:
\[ Q = \Delta U \]

**Hint:** When work done is zero, the heat added to the system equals the change in internal energy.

### Step 4: Conclusion
The heat change of a process in which the volume remains constant is represented by:
\[ Q = \Delta U \]
This means that the heat change (Q) is equal to the change in internal energy (ΔU).

**Hint:** Look for the relationship between heat and internal energy when volume is constant.

### Final Answer
The correct representation of the heat change of a process in which volume remains constant is:
**ΔU** (Option 1).