Certainly! Here is the transcription and explanation suitable for an educational website:---**Problem Statement:**5. Calculate the approximate final temperature of water in a coffee cup calorimeter if 33.9 kJ of heat is added to 420.0 g of water initially at a temperature of 22.60 °C (the specific heat of water is 4.184 J/g·K).**Explanation:**This problem involves calculating the final temperature of water after a specified amount of heat energy is added to it. The process is done using a coffee cup calorimeter, which is an apparatus used to measure the heat of chemical reactions or physical changes.**Relevant Formula:**To find the final temperature, we use the formula:\[ q = m \cdot c \cdot \Delta T \]Where:- \( q \) is the heat added (in joules),- \( m \) is the mass of the water (in grams),- \( c \) is the specific heat capacity of water (in J/g·K),- \( \Delta T \) is the change in temperature (in °C or K).**Steps to Solve:**1. **Convert Heat Energy to Joules:** - Since 1 kJ = 1000 J, convert heat from kJ to J. - \( 33.9 \, \text{kJ} = 33,900 \, \text{J} \)2. **Apply the Formula:** - Rearrange the formula to solve for \( \Delta T \): \[ \Delta T = \frac{q}{m \cdot c} \]3. **Insert Known Values:** - \( q = 33,900 \, \text{J} \) - \( m = 420.0 \, \text{g} \) - \( c = 4.184 \, \text{J/g·K} \) - Calculate \( \Delta T \).4. **Calculate Final Temperature:** - \( \Delta T = \frac{33,900 \, \text{J}}{420.0 \, \text{g} \times 4.184 \, \text{J/g·K}} \) - \( \Delta T \approx 19.28 \, \text{K} \)5. **Determine Final

Use calorimetry principle to get answer Heat flow from high temperature to low temperature. Heat=…

5. Calculate the approximate final temperature of water in a coffee cup calorimeter if 33.9 kJ of heat is added to 420.0 g of water initially at a temperature of 22.60 °C (the specific heat of water is 4.184 J/g•K).

5. Calculate the approximate final temperature of water in a coffee cup calorimeter if 33.9 kJ of heat is added to 420.0 g of water initially at a temperature of 22.60 °C (the specific heat of water is 4.184 J/g•K).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

33.79 g of a solid is heated to 100.°C and added to 50.0 g of water in a coffee cup calorimeter and the contents are allowed to sit until they finally have the same temperature. The water temperature changes from 29.76 °C to 38.3 °C and the specific heat capacity of water is 4.184J/g °C. What is the specific heat capacity (in J/g°C) of the solid? O 1.73 O 1.17 O 0.857 O 0.579
When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175.0 g of water was placed in a coffee-cup calorimeter and chilled to 10.0 °C. Then 49.0 g of pure sulfuric acid, also at 10.0 °C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9 °C. Assume that the specific heat capacity of the resulting sulfuric acid solution is 4.19 J/g °C. Calculate the quantity of thermal energy transferred, Q, for the formation of this solution, and calculate the molar enthalpy of solution in kilojoules per mole of H₂SO4.
6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).
30 g of HCL is mixed with 200 g of water. The water temperature changes from 24.6 to 28.2 °C. What was the heat change (enthalpy change) of the water?
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat
When 14.2 g KBr is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature drops from 28.88 °C to 23.38 °C. What is the enthalpy change per gram of KBr dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g·K.
A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt? How many moles of the unknown salt were used in the reaction ? _______ J?
4. Determine the final temperature of water if 9.2 kJ of heat is added to 250 mL of 17°C water (the specific heat capacity of water is 4.184 J/g°C).
A sample of aluminum, initially at 5.0 °C, was placed in 18.0 g of water, initially at 25.0 °C. The final temperature of the water and the metal was 21.0 °C. The specific heat of water is 4.184 J g-1 °c-1 and aluminum is 0.940 J g-1 °C-1. Ignore the heat capacity of the container. What is the mass (in g) of the aluminum?
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
3. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal.