The reaction described takes place in solution in a coffe-cup style calorimeter. We will assume that the cups absorb or release a negligible amount of heat so we will not need to worry about the calorimeter constant or qcal.
If the total mass of the solution in the calorimeter is 23.03 g and and the solution increases from 15.21 °C to 53.67 °C, what is the value of q in joules for the reaction. Include the correct sign with your value of q. C = 4.179 J/g°C for the solution.
well, if the temp rose, the reaction was exothermic (negative sign).
heat=-23.03*C*(53.67-15.21)
To calculate the value of q for the reaction, we can use the formula:
q = m * C * ΔT
Where:
- q is the heat transferred in joules (J)
- m is the mass of the solution in grams (g)
- C is the specific heat capacity of the solution in joules per gram per degree Celsius (J/g°C)
- ΔT is the change in temperature in degrees Celsius (°C)
Given:
- m = 23.03 g
- C = 4.179 J/g°C
- ΔT = 53.67 °C - 15.21 °C = 38.46 °C
Plugging in the values into the formula:
q = 23.03 g * 4.179 J/g°C * 38.46 °C
Now, let's calculate the value of q:
q = 3826.875 J
Since the solution increased in temperature, it means heat was absorbed by the solution. Therefore, the sign of q is positive (+3826.875 J).