Enter your answer in the provided box. A sheet of gold weighing 11.4 g and at a temperature of 11.4°C is placed flat on a sheet of iron weighing 19.5 g and at a temperature of 50.6°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings.

Enter your answer in the provided box. A sheet of gold weighing 11.4 g and at a temperature of 11.4°C is placed flat on a sheet of iron weighing 19.5 g and at a temperature of 50.6°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g...

See similar textbooks

Related questions

Q: A sheet of gold weighing 10.0 g and at a temperature of 18.0°C is placed flat on a sheet of iron…

Q: In the laboratory a student finds that it takes 75.4 Joules to increase the temperature of 13.3…

A: Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg…

Q: When 151.0 mL of water at 26.0 C is mixed with 71.0 mL of water at 85.0 C, what is the final…

Q: In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used…

A: Mass of copper, MCu = 60.04 g Mass of water, Mw = 79.22 g Initial temperature of Copper, TCu = 97.70…

Q: The specific heat capacities for several substances are shown in the table. Substance Specific Heat…

A: We have to predict which substance wil undergo greatest temperature change .

Q: Enter your answer in the provided box. A gas expands and does P-Vwork on the surroundings equal to…

Q: The heat capacity of a sample should be divided by which quantity to find the specific heat…

A: When Heat capacity is divided by mass in grams we get specific heat capacity.

Q: Enter your answer in the provided box. A sheet of gold weighing 9.6 g and at a temperature of 13.6°C…

A: Given, Mass of Gold, mAu = 9.6 g Temperature, TAu = 13.6 °C Mass of iron, mFe = 18.0 g…

Q: Which of the following statements is always true? a. The change in temperature in degrees Celsius…

A: Temperature is the measure of hotness and coldness of a body

Q: Which of the following is the correct definition of enthalpy? Enthalpy is the heat of combustion.…

A: The enthalpy can be written asΔH = ΔU + PΔV Where ΔU is the change in the internal energyP is the…

Q: A 20.8 g piece of metal has a specific heat of 0.52 J/g°C. It was heated to 9.5°C then placed inside…

A: Formula used : -q(lost) = q(gained) If no heat is lost to the surrounding.

Q: the laboratory a student finds that it takes 29.3 Joules to increase the temperature of 13.1 grams…

A: Given -> ∆H= 29.3 joule Weight (m) = 13.1 gm T1=20.0°C T2= 37.9°C

Q: A sheet of gold weighing 9.3 g and at a temperature of 17.6°C is placed flat on a sheet of iron…

A: Given: mgold =9.3 g CAu = 0.129 J/g 0C Ti = 17.6 0C miron =21 g CFe = 0.444 J/g 0C Tiron = 55.3 0C…

Q: The mixture of gas and air inside a cylinder reacts, releasing 400kJ total energy. If the system…

A: Given: The total energy is 400 kJ. The work done by system is 250 kJ.

Q: Which of the following statements is/are CORRECT? 1. A system is defined as an object or collection…

A: The Thermodynamics is the study of heat inside the system. The system is subject to change in terms…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 446.0 mg sample…

Q: How much heat is given off to the surroundings when 7 g of aluminum reacts according to the…

A: The enthalpy of the reaction is considered as the state function that is it depends only on the…

Q: A student heats 68.15 grams of silver to 98.73 °C and then drops it into a cup containing 78.21…

A: All the information is given in question Mass of silver and temperature Mas software water and…

Q: A hot lump of 29.8 g of copper at an initial temperature of 50.7 °C is placed in 50.0 mL H2O…

A: Given data is: Mass of copper = 29.8 g Initial temperature = 50.7°C Mass of water = 50.0 ml Density…

Q: How many milliliters of water at 3.16°C with a density of 1.00 g/mL must be mixed with 180 mL (about…

Q: piece of unknown metal with a mass of 24.31 g is heated in boiling water to 90.51°C and then dropped…

A: The solution is provided in the next step: Given data: * Mass of metal is 24.31 g. * Mass of water…

Q: A 312 g sample of a metal is heated to 281.562 °C and plunged into 200 g of water at a temperature…

A: Here we can calculate the heat gained by water using its specific heat , mass and temperature…

Q: Which of the following makes sense: When volume of a system is under constant pressure, which of…

A: The enthalpy change is defined as the internal energy change plus product of constant pressure and…

Q: A sheet of gold weighing 9.3 g and at a temperature of 15.2°C is placed flat on a sheet of iron…

A: Since both the metals are in contact hence the heat will transfer from the hot sheet to cold sheet…

Q: When 126.0 mL of water at 26.0 ° C is mixed with 66.0 mL of water at 85.0 ° C, what is the final…

A: Given are two samples of water. The mass of water in two samples can be calculated as

Q: A student heats 61.27 grams of silver to 97.71 °C and then drops it into a cup containing 82.16…

Q: A 2.57 g sample of a substance suspected of being pure gold is warmed to 72.9 °C and submerged into…

Q: The specific heat capacities for several substances are shown in the table. Substance Specific Heat…

A: Given :- Substance specific heat (J/g°C) Iron 0.45 Air…

Q: A 55.0g sample of metal z requires 675j of energy to heat it from 25.0 to 118.0 Celsius? Calculate…

Q: When 156.0 mL of water at 26.0°C is mixed with 86.0 mL of water at 85.0°C, what is the final…

A: Convert the given mL of water into mass.Given, density of water = 1.00 g/mL

Q: An unknown substance requires 567 J of heat to increase its temperature from 0 to 15 ºC. The sample…

A: Given, Amount of heat required (Q) = 567 J Initial temperature (Ti) = 0°C Final temperature (Tf) =…

Q: A sheet of gold weighing 9.8 g and at a temperature of 17.8°C is placed flat on a sheet of iron…

A: Given information: Mass of gold = 9.8 g Temperature for gold = 17.8∘C mass of iron = 20.3 g…

Q: A 20.94 g sample of a metal is heated to 99.4°C in a hot water bath until thermal equilibrium is…

A: The heat lost by the metal is determined as follows,

Q: When 375 mL of water (d = 1.00g/mL) at 32°C are mixed with 125 mL of water at 92°C, what is the…

A: Mass of 375 mL water and 125 mL water is calculated as follows,

Q: A pure sample of Substance S is put into an evacuated flask. The flask is then heated steadily and…

A: For substance Y and Z , those parts of graph will change as per substance S which are different .…

Q: An unknown hot metal at 122.41°C with a mass of 53.37g was mixed with 28.15g of water at an initial…

A: We have to calculate the specific heat of the unknown metal.

Q: An unknown solid metal at 150 degrees celsius was placed in 1.00 L of water at 25 degrees celsius.…

A: Heat absorbed or emitted by a substance = mass of the substance x specific heat of the substance x…

Q: A hot lump of 33.8 g of iron at an initial temperature of 51.8 C is placed in 50.0 mL H,0 initially…

Q: Enter your answer in the provided box. A sheet of gold weighing 10.0 g and at a temperature of…

Q: 27-gram piece of metal at 144 oC is dropped into 86 grams of water at 29 oC. The water temperature…

Q: A piece of unknown metal with a mass of 23.78 g is heated in boiling water to 97.4°C and then…

A: Specific heat of substance defined as the heat capacity of sample of substance is divided by…

Q: When 2 mol of potassium chlorate crystals decompose to potassium chloride crystals and oxygen gas at…

A: A thermochemical equation for a given reaction can be defined as the balanced stoichiometric…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 506.0 g sample…

A: Given Mass (m)= 506.0 g Initial temperature (Ti) = -2.4 °C Final temperature (Tf) = 21.6 °C Heat…

Q: A sheet of gold weighing 10.6 g and at a temperature of 15.3°C is placed flat on a sheet of iron…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.57 kg sample…

Q: Calculate the specific heat of a metal if 45.0 grams of the metal at 100.0 °C, when placed into…

Q: How much heat is given off to the surroundings when 6 g of aluminum reacts according to the…

A: Thermodynamics is the branch of chemistry that mainly deals with the heat transfer between system…

Question

Enter your answer in the provided box.
A sheet of gold weighing 11.4 g and at a temperature of 11.4°C is placed flat on a sheet of iron weighing
19.5 g and at a temperature of 50.6°C. What is the final temperature of the combined metals? Assume
that no heat is lost to the surroundings.
°C

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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 oC.
A block of aluminum and a block of iron, both having the same mass, are removed from a freezer and placed outside on a warm day. When the same quantity of heat has flowed into each block, which block will be warmer? Assume that neither block has yet reached the outside temperature. (See Table 6.1 for the specific heats of the metals.)
A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed in a container of water at 22.3C. The final temperature of the water and copper is 24.9C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?
If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)
Swimming Pool A swimming pool measuring 20.0m12.5m is filled with water to a depth of 3.75m. If the initial temperature is 18.4°C, how much heatmust be added to the water to raise its temperature to29.0°C? Assume that the density of water is 1.000 g/mL.
Determine whether the statements given below are true or false. Consider an endothermic process taking place in a beaker at room temperature. (a) Heat flows from the surroundings to the system. (b) The beaker is cold to the touch. (c) The pressure of the system decreases. (d) The value of q for the system is positive.
An aluminum kettle weighs 1.05 kg. (a) What is the heat capacity of the kettle? (b) How much heat is required to increase the temperature of this kettle from 23.0 C to 99.0 C? (c) How much heat is required to heat this kettle from 23.0 C to 99.0 C if it contains 1.25 L of water (density of 0.997 g/mL and a specific heat of 4.184 J/g C)?
The Group 2A carbonates decompose when heated. For example, MgCO3(s)MgO(s)+CO2(g) Use enthalpies of formation (see Appendix C) and calculate the heat required to decompose 10.0 g of magnesium carbonate.
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
You have two samples of different metals, metal A and metal B, each having the same mass. You heat both metals to 95C and then place each one into separate beakers containing the same quantity of water at 25C. a You measure the temperatures of the water in the two beakers when each metal has cooled by 10C and find that the temperature of the water with metal A is higher than the temperature of the water with metal B. Which metal has the greater specific heat? Explain. b After waiting a period of time, the temperature of the water in each beaker rises to a maximum value. In which beaker does the water temperature rise to the higher value, the one with metal A or the one with metal B? Explain.
Given the following (hypothetical) thermochemical equations: A+B2C;H=447kJA+3D2E;H=484kJ2D+B2F;H=429kJ Calculate H, in kJ, for the equation 4E+5B4C+6F
9.30 For the example of shallow water and sandy beaches, which material has a larger heat capacity or specific heat? How does a hot day at the beach provide evidence for your answer?