As a result of the isobaric change by 80 K, one mole of a certain ideal gas obtain an amount of heat equal to 1.60 kJ.
What is value of `C_(P)(JK^(-1))`?

Options

A. 1.6
B. 16
C. 20
D. 2

Explanation

To solve the problem, we need to determine the value of \( C_P \) (heat capacity at constant pressure) for one mole of an ideal gas, given the amount of heat absorbed and the temperature change.

### Step-by-Step Solution:

1. **Identify the Given Values:**
- Amount of heat absorbed, \( Q = 1.60 \, \text{kJ} = 1600 \, \text{J} \) (since \( 1 \, \text{kJ} = 1000 \, \text{J} \))
- Temperature change, \( \Delta T = 80 \, \text{K} \)

2. **Understand the Relationship:**
- The heat capacity at constant pressure \( C_P \) is defined as:
\[ C_P = \frac{Q}{\Delta T} \]
- Here, \( Q \) is the heat added and \( \Delta T \) is the change in temperature.

3. **Substitute the Values:**
- Now, substitute the values of \( Q \) and \( \Delta T \) into the formula:
\[ C_P = \frac{1600 \, \text{J}}{80 \, \text{K}} \]

4. **Calculate \( C_P \):**
- Performing the division:
\[ C_P = 20 \, \text{J/K} \]

5. **Final Result:**
- Therefore, the value of \( C_P \) is \( 20 \, \text{J/K} \).