How do I solve this? How much heat (in Joules) is gained by the water when a chemical reaction takes place in 100.0 ml aqueous solution, has a temperature increase of 12.67°C and a specific heat capacity of 4.180 J/°Cg? [Hint: ignore any effects of the calorimeter and solve for qwater]
To solve this question, you need to calculate the heat gained by the water during the chemical reaction. The heat gained or lost can be determined using the equation:
q = m * c * ΔT
where:
q = heat gained or lost
m = mass of the substance (water)
c = specific heat capacity of the substance (water)
ΔT = change in temperature
Given:
- Volume of the aqueous solution = 100.0 mL
- Density of water = 1 g/mL (approximately)
- Mass of the solution = volume * density = 100.0 g
- Specific heat capacity of water = 4.180 J/°Cg
- Temperature increase = 12.67 °C
Now, substitute these values into the equation:
q = (100.0 g) * (4.180 J/°Cg) * (12.67 °C)
q = 5348.17 J
Therefore, the water gains 5348.17 Joules of heat during the chemical reaction.