An insulated calorimeter contains 100 g of water at 22 °C. A chemical reaction causes the temperature to increase by 6 °C. Given that water has a specific heat of 4.184 J/g°C, how much heat was transferred to or from the water? Group of answer choices-2.5 kJ-1.5 kJ-2.0 kJ-1.0 kJ
Question
An insulated calorimeter contains 100 g of water at 22 °C. A chemical reaction causes the temperature to increase by 6 °C. Given that water has a specific heat of 4.184 J/g°C, how much heat was transferred to or from the water? Group of answer choices-2.5 kJ-1.5 kJ-2.0 kJ-1.0 kJ
Solution
To calculate the heat transferred, we can use the formula for heat transfer which is:
q = mcΔT
where:
- q is the heat transferred
- m is the mass of the substance (in this case, water)
- c is the specific heat of the substance
- ΔT is the change in temperature
Given:
- m = 100 g
- c = 4.184 J/g°C
- ΔT = 6°C
Substituting these values into the formula, we get:
q = (100 g) * (4.184 J/g°C) * (6°C) = 2510.4 J
Since 1 kJ = 1000 J, we can convert this to kJ:
2510.4 J = 2.51 kJ
So, the heat transferred to the water is approximately 2.5 kJ.
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