A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 7.40kg of water at 23.4°C. During the reaction 104.kJ of heat flows out of the bath and into the flask.Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g−1K−1. Be sure your answer has the correct number of significant digits.°C
Question
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 7.40kg of water at 23.4°C. During the reaction 104.kJ of heat flows out of the bath and into the flask.Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g−1K−1. Be sure your answer has the correct number of significant digits.°C
Solution
To solve this problem, we need to use the formula for heat transfer:
q = mcΔT
where: q = heat energy (in joules) m = mass (in grams) c = specific heat capacity (in joules per gram per degree Celsius) ΔT = change in temperature (in degrees Celsius)
First, we need to convert the mass of the water from kg to g, because the specific heat capacity is given in J/g·K.
7.40 kg = 7400 g
Next, we need to convert the heat energy from kJ to J, because the specific heat capacity is given in J/g·K.
104 kJ = 104000 J
Now we can plug the values into the formula and solve for ΔT:
104000 J = 7400 g * 4.18 J/g·K * ΔT
Rearranging the equation to solve for ΔT gives:
ΔT = 104000 J / (7400 g * 4.18 J/g·K) = 3.35°C
The heat flowed out of the bath and into the flask, so the water bath cooled down. Therefore, the final temperature of the water bath is the initial temperature minus the change in temperature:
23.4°C - 3.35°C = 20.05°C
So, the new temperature of the water bath is 20.05°C.
Similar Questions
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
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celcius is added to 50.00 grams of water initially at 10.67 degrees Celcius. The final temperature of the system is 20.15 degrees Celcius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C).
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.28kg sample of a pure substance from 11.1°C to 17.0°C. The experiment shows that 14.kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits.
A sample of water was heated and allowed to cool down. The energy transferred to the surroundings was 132 300 J and the temperature changed from 70 °C to 25 °C.The specific heat capacity of water is 4200 J/kg°C.What was the mass of the sample of water?You must include units with your answer.
A 44.0g sample of glass, which has a specific heat capacity of 0.670·J·g−1°C−1, is dropped into an insulated container containing 200.0g of water at 65.0°C and a constant pressure of 1atm. The initial temperature of the glass is 8.2°C.Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has the correct number of significant digits.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.