**Physics Problem: Heat Transfer Calculation****Problem Statement:**The specific heat of iron is \(0.4494 \, \text{J/g} \cdot °\text{C}\). How much heat is transferred when a \(4.7 \, \text{kg}\) piece of iron is cooled from \(180 \, °\text{C}\) to \(13 \, °\text{C}\)?---To solve this problem, consider using the formula for heat transfer:\[q = m \cdot c \cdot \Delta T\]Where:- \(q\) is the heat transferred (in Joules),- \(m\) is the mass of the substance (in grams),- \(c\) is the specific heat capacity (in Joules per gram per degree Celsius),- \(\Delta T\) is the change in temperature (in degrees Celsius).Convert the mass from kilograms to grams:\[4.7 \, \text{kg} = 4700 \, \text{g}\]Calculate the change in temperature:\[\Delta T = T_{\text{final}} - T_{\text{initial}} = 13 \, °\text{C} - 180 \, °\text{C} = -167 \, °\text{C}\]Substitute these values into the formula to find the heat transferred.

Answered: Image /qna-images/answer/c1fc99bd-8bf7-4b9e-b7cf-20ee3b465feb.jpg

Answered: 2. The specific heat of iron is 0.4494…

2. The specific heat of iron is 0.4494 J/g x °C. How much heat is transferred when a 4.7 kg piece of iron is cooled from 180 °C to 13 °C?

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

A 234.66 gram aqueous solution has a specific heat of 4.186 J/gºC. The solution is at 28.1 °C. What is the temperature of the solution in °C after 54.93 kJ of heat has been added to it?
A student is asked to identify an unknown piece of metal. The metal has a mass of 12.34 g. It is placed in a boiling water bath and brought up to 99.98 oC. A coffee-cup calorimeter is set up with 103.25 mL of water (density = 1.00 g/mL and specific heat = 4.184 J/g.oC) at a room temperature of 21.30 oC. The metal is removed from the boiling water and placed in the calorimeter. A final temperature is recorded as 22.32 oC. Find the specific heatcapacity of the unknown metal. (Assume there is no heat loss)
6. Calculate the amount of heat released when 1.26 x 104 grams of ammonia NH3 are produced according to the following equation. N₂ + 3H₂ → 2NH3 AH = -92.6 kJ
specific heat of gold is 0.129J/g C. what is molar heat capacity of gold?
What is the specific heat of a 45.51 g piece of an unknown metal that exhibits a 45.2 °C temperature change upon absorbing 1870 J of heat?
a 90.00g piece of metal is placed in water and the water gains 1230 J of heat as the temperature of the metal changes by 59.0 C. calculate the specific heat capacity of the metal
1
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
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).
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?
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.