Calculate the change in temperature, Delta t that occurs when 12.0 kJ of thermal energy is added to 0.350 kg of water. (look in the data sheet for the specific heat capacity for water, unit conversions, do NOT include units) square A

Here's how to calculate the change in temperature:<br /><br />1. **Find the specific heat capacity of water:** The specific heat capacity of water is 4.18 kJ/kg°C (this value should be provided in a data sheet or can be easily looked up).<br /><br />2. **Use the formula for heat transfer:** The formula relating heat transfer (Q), mass (m), specific heat capacity (c), and change in temperature (Δt) is: Q = mcΔt<br /><br />3. **Rearrange the formula to solve for Δt:** Δt = Q / (mc)<br /><br />4. **Plug in the values:** Δt = 12.0 / (0.350 * 4.18)<br /><br />5. **Calculate:** Δt ≈ 8.196<br /><br />Therefore, the change in temperature is approximately 8.20. Since the question specifically states to *not* include units, the answer is simply **8.20**.<br />