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The problem asks you to calculate the energy required to heat 0.90 kg of ethanol from 0.4°C to 14.3°C, given the specific heat capacity of ethanol is 2.44 J·g⁻¹·K⁻¹.

We can solve this using the heat energy formula:

\[
Q = mc\Delta T
\]

Where:
- \(Q\) is the heat energy (in joules).
- \(m\) is the mass (in grams) of ethanol.
- \(c\) is the specific heat capacity (in J·g⁻¹·K⁻¹).
- \(\Delta T\) is the change in temperature (in °C or K).

### Step 1: Convert mass to grams
Since \( m = 0.90 \, \text{kg} = 900 \, \text{g} \).

### Step 2: Calculate the temperature change (\(\Delta T\))
\[
\Delta T = 14.3 \, \text{°C} - 0.4 \, \text{°C} = 13.9 \, \text{°C}
\]

### Step 3: Plug values into the heat energy formula
\[
Q = 900 \, \text{g} \times 2.44 \, \text{J·g}^{-1}·\text{K}^{-1} \times 13.9 \, \text{K}
\]

### Step 4: Perform the calculation
\[
Q = 900 \times 2.44 \times 13.9 = 30,502.8 \, \text{J}
\]

Rounding to 3 significant figures (based on the given data), the energy required is:

\[
Q \approx 30,500 \, \text{J}
\]

Would you like more details or have any questions?

Here are 5 related questions to explore:
1. What would the energy be if the mass of ethanol was doubled?
2. How does the specific heat capacity of ethanol compare to water?
3. What happens if the final temperature was higher than 14.3°C?
4. What are the units of specific heat capacity and why are they important?
5. How is heat energy related to phase changes in substances?

**Tip:** Always keep track of units during calculations to ensure accuracy.

Calculate the energy required to heat 0.90 kg of ethanol from 0.4 °C to 14.3 °C. Assume the specific heat capacity of ethanol under these conditions is 2.44 J·g⁻¹·K⁻¹.

Learn how to calculate the energy required to heat 0.90 kg of ethanol from 0.4°C to 14.3°C using the specific heat capacity formula. This problem involves thermodynamic concepts and unit conversions, suitable for students in Grades 10-12.

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