**Heat Transfer Calculation in Automobile Radiators****Problem Overview:**The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator, the temperature drops to 175 °F. We need to calculate the amount of heat transferred from the engine to the surroundings by one gallon of water. The specific heat capacity of water is 4.184 J/g°C.**Steps to Solve the Problem:**1. **Convert Temperatures to Celsius:** - Use the conversion formula: \( °C = (°F - 32) \times \frac{5}{9} \). - Convert 240 °F and 175 °F to Celsius.2. **Calculate the Change in Temperature (ΔT):** - Find the difference between the initial and final temperatures in Celsius.3. **Determine the Mass of Water:** - Find the mass of one gallon of water in grams.4. **Calculate Heat Transferred (q):** - Use the formula: \( q = m \times c \times ΔT \), where \( m \) is the mass of the water, \( c \) is the specific heat capacity, and \( ΔT \) is the temperature change.**Note:** Ensure all units are consistent, particularly when converting temperatures and calculating heat in Joules, to obtain accurate results.

Amount of heat transferred Q = mCΔT Given - - > Initial temperature = 240 °F = 115.56°C We know…

The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator it has a temperature of 175 °F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g °C. Type your answer. Next Previous

The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator it has a temperature of 175 °F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g °C. Type your answer. Next Previous

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

It is assumed that the heat given up by the metal is transferred to the water. The specific heat of water is 4.18 J/g°C, which means that 4.18 Joules of heat energy is required to raise the temperature of 1 gram of water 1 °C. Use the table below to determine which metal your unknown is. Metal Specific Heat (J/g°C) Aluminum 0.902 Brass 0.380 Copper 0.385 Gold 0.126 Iron 0.449 Nickel 0.444 Silver 0.235 Fill out the table below and determine the identity of the unknown metal.
In the lab, a cube of wood has a mass of 35.8 grams and its temperature rises from 20.3oC to 79.5oC when placed outside in the sun for a period of time. Calculate the amount of heat absorbed by the wood. The specific heat of wood is 1.76 J/goC .
A gold bar of unknown amount absorbs 1.09 kJ of heat and raises its temperature from 5.3 °C to 72.2 °C. What is the mass (g) of the gold piece? The specific heat and density of gold are 0.128 J/g°C and 19.32 g/cm3
The specific heat of copper is 0.385 J/g°C. Calculate the final temperature when 25.0 g of copper metal at 100°C is added to 50 mL of water at 20°C.
When a 1.44-g sample of magnesium metal is burned, it produces enough heat to raise the temperature of 1,617 g of water from 24.00°C to 33.10°C. How much heat did the magnesium release when it burned? (The specific heat of water is 4.184 J/g·°C.)
you apply 37.0 kj of heat energy to 155 grams of water 25 celsius. does the water boil? if not what is the temperature of water at 40.7 kj
Some homes that use baseboard heating use copper tubing. Hot water runs through and heats the copper tubing, which in turn heats aluminum fins. It is actually the aluminum fins that heat the air rising through the fins. How much energy would it take to heat a section of the copper tubing that weighs about 595.0 g , from 13.61 °C to 23.64 °C ? Copper has a specific heat of 0.3850 (J/g) · °C. Express your answer to four significant figures. • View Available Hint(s) ΑΣφ ? Heat = J
In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a metal.She heats 19.2 grams of magnesium to 98.96°C and then drops it into a cup containing 77.8 grams of water at 22.66°C. She measures the final temperature to be 27.15°C.Assuming that all of the heat is transferred to the water, she calculates the specific heat of magnesium to be ________ J/g°C.
A solution is made by mixing 260.0 mL of ethanol initially at 15.5 °C with 260.0 mL of water initially at 23.4 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g.°C and the specific heat of water is 4.184 J/g.°C. Tf = °C
How much heat is required to raise the temperature of 25g of water from 25.0°C to 30.0°C? The specific heat of water is 4.184J/g°C.
R Please don't provide the handwriting solution
A beaker of hot water with a volume of 43.9 mL has an initial temperature of 94.3 °C. You place a block of metal that has a mass of 43.89 g into the water until the water and metal are at thermal equilibrium. You record that the temperature of the metal increases by 66.56 °C. What is the final temperature °C at thermal equilibrium of the water and block, assuming no heat is lost to the surroundings? The specific heat of the metal block is 0.237 J/g·°C