2) The specific heat capacity of iron is 0.461 J/g K and 0.544 J/g K for titanium. A sample consisting of a mixture of 10.0g Fe and 10.0g Ti at 100.0 °C loses 200 J of heat to the environment. What is the final temperature of the sample? a. 89.9 °C b. 80.1 °C c. 60.2 °C d. 39.8 °C

2) The specific heat capacity of iron is 0.461 J/g K and 0.544 J/g K for titanium. A sample consisting of a mixture of 10.0g Fe and 10.0g Ti at 100.0 °C loses 200 J of heat to the environment. What is the final temperature of the sample? a. 89.9 °C b. 80.1 °C c. 60.2 °C d. 39.8 °C

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 107QRT: The specific heat capacity of copper is 0.385 J g1 C1, whereas it is 0.128 J g1 C1 for gold. Assume...

See similar textbooks

Related questions

Q: One tablespoon of cookie dough has a mass of 14.69 g. It is combusted in a calorimeter whose heat…

A: q = m. C. ∆T q = heat in joules m = mass in grams ∆T = Tf - Ti = final temperature - initial…

Q: A piece of metal with mass 20.00 g at room temperature [25.0oC] was heated up to 90.0oC. This metal…

A: a) The amount of heat water gained is given by Q as Q = mCΔT where m = mass of water = density X…

Q: 7.00 Jof heat is added to 10.00g of gold, which is initially at 25°C. The heat capacity of gold is…

Q: A piece of silver, with specific heat capacity of 0.235 J/(g.°C), is added to an insulated container…

A: Given: The specific heat of water, (cH2O) =4.184 J(g. 0C). The specific heat of silver, (cAg) =…

Q: 15 The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental…

A: Given reaction and information, 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) ΔH = –850. kJ

Q: A 8.17 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

Q: A beaker contained 76.4 g of water at 18.97°C. A 85.48-g sample of metal at 51.36°C was placed in…

A: Given that Mass of water = 76.4 g Mass of metal = 85.48 g Initial temperature of water = 18.97°C…

Q: A piece of calcite is heated to 72.0°C and placed in a styrofoam coffee cup containing 25.0 mL of…

A: GIVEN: The temperature of Calcite=72.0°C Volume of water= 25.0 mL The initial temperature of water=…

Q: A 356 g sample of nitrogen goes through a temperature change of +71.43 °C. The J specific heat…

Q: Determine the amount of heat needed to raise a piece of metal 54.8 K. The piece of metal has a mass…

Q: To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of…

Q: Consider the following specific heats of metals. Metal Specific Heat сopper 0.385 J/(g•°C) magnesium…

A: Heat capacity is amount of heat required to raise the temperature of substance by one degree…

Q: A chemist measures the energy change AH during the following reaction: 2 Fe, O3(s) 4 FeO(s)+O,(9)…

A: We have to predict the nature of reaction, heat absorbed, amount of heat absorbed.

Q: A chunk of iron at 90.6°C was added to 200.0 g of water at 15.5°C. The specific heat of iron is…

A: Given: Mass of water = 200.0 g. Initial temperature of water = 15.5 oC Final temperature of mixture…

Q: Calorimeter Y has a greater heat capacity than Calorimeter Z. What does this imply? Select one: O a.…

A: Given heat capacity of calorimeter Y is greater than calorimeter Z

Q: 5.4.1 A 1.000-g sample of benzoic acid is burned in a calorim-eter to determine its heat capacity,…

A: The heat capacity of the calorimeter has to be calculated,

Q: Silicon, used in computer chips, has a heat capacity of 0.712 J·g-1·°C-1. If 500 J of heat is…

A: Given: Heat capacity of silicon = 0.712 J g-1 °C-1 Absorbed heat = 500 J Mass of silicon = 8.13 g…

Q: 2. An aluminum container with specific heat capacity of 0.880 J/g"C contains waxwith specific heat…

A: Please find the attached images for the answer I am giving the answer for question number 2 only.

Q: A 0.6575−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat…

A: The heat given by 0.6575 g of Mg to the calorimeter (q) is calculated using equation (1) where C is…

Q: energy (in joules) is needed to heat 200.0 g of water by 10.0 C? The heat capacity of water is…

A: The energy in joules that is needed to heat 200.0 g of water by 10.0 degrees Celsius is to be…

Q: One tablespoon of cookie dough has a mass of 13.02 g13.02 g. It is combusted in a calorimeter whose…

Q: Ice at 0°C is placed in a Styrofoam cup containing 361 g of a soft drink at 23°C. The specific heat…

A: Answer:- This question is answered by using the simple concept of calorimetry which states that heat…

Q: A chunk of lead at 91.6°C was added to 200.0 g of water at 15.5°C. The specific heat of lead is…

A: We know that, according to the law of conservation of heat energy, energy gained or loss by the…

Q: LP gas burns according to the exothermic reaction:C3H8(g) + 5 O2(g) -------->3 CO2(g) + 4…

Q: 16.) A 45.0 g silver spoon was submerge to a 200 g of coffee drink in a 432 g ceramic mug. If the…

Q: Aluminum metal reacts with chlorine with a display of sparks: 2 Al(s) + 3 Cl2(g) ➜ 2 AlCl3(s)…

A: In the given reaction, 2 Al(s) + 3 Cl2 (g) ➜ 2 AlCl3 (s) ΔH = –1408 kJ

Q: 100 g of water at 86 °C is mixed with 200 g of water at 17 °C. What is the final temperature of the…

A: apply the concept , heat taken = heat given

Q: To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of…

Q: 1. A 5.000 g sample of methanol, CH,OH, was combusted in the presence of excess oxygen in a bomb…

A: given information from question are- mass of methanol = 5g. mass of water = 4000 g. temperature…

Q: A pyrex glass flask is filled with 200 g of water. The energy required to heat the system (the flask…

Q: Calorimeter Y has a greater heat capacity than Calorimeter Z. What does this imply? Select one: a.…

A: Heat capacity is defined as the amount of heat required to rise the temperature of calorimeter…

Q: beaker contained 69.68 g of water at 15.25°C. A 81.2-g sample of metal at 52.22°C was placed in it,…

Q: 150. g of water (Cs = 4.184 J/g°C) at 20.0 °C is added to a coffee cup calorimeter. A 35.0 g sample…

A: We use conservation of heat law in order to achieve equilibrium :- -Heat released by the solid =…

Q: The highly exothermic thermite reaction, in which aluminum reduces iron(ll) oxide to elemental iron,…

A: Heat released and absorbed in a chemical reaction is function of the numbe of moles of reactants…

Q: A 100.0 g sample of an unknown metal is heated to 95.00°C. This hot metal is then placed into a foam…

Q: To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of…

Q: A 17.1 g piece of silver was heated to 98.8 °C in boiling water and then dropped into a beaker…

Q: A 7.50 g marshmallow is placed in a calorimeter and burned in excess oxygen. The temperature…

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

Q: A 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then…

A: The amount of heat transferred in a thermodynamic system is calculated as follows,…

Q: A 7.50 g marshmallow is placed in a calorimeter and burned in excess oxygen. The temperature…

A: Since whatever energy was released by burning the marshmallow is used to rise the temperature of…

Q: 1. Consider the following data: Metal AI Cu Mass (g) Specific heat (J/g °C) | 0.9 Temperature (°C)…

Q: 15.0 J of heat is added to 10.00 g of gold, which is initially at 25°C. The heat capacity of gold…

A: Given: Heat energy (Q) = 15.0 J Mass of metal (m) = 10.0 g Initial temperature of metal = 25.0 oC…

Q: A metal with a specific heat of 0.899 J/g oC had an initial temperature of 76.67 oC. When it was…

A: The heat transferred during the reaction can be determined from the given equation. The temperature…

Q: A flask containing 1059 g of water is heated and a temperature increase from 32.4 °C to 67.6 °C. How…

A: The mass of one mole of water is = 18 g The initial temperature of the water is = 32.4oC The final…

Q: An 8.0 g sample margarine was placed in a bomb calorimeter. It was then completely combusted leading…

A: Ans Heat change in bomb calorimetry is given by the formula DeltaH = mc(T2-T1) Now given values…

Q: A 158 g sample of gold at some temperature was added to 28.7 g of water. The initial water…

A: Assuming the initial temperature of gold is T. Since the heat lost by gold is gained by water to…

Q: The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental…

A: Heat is arises due to change in temperature and heat is transferred from hotter body to colder body.…

Q: When a reaction that was known to release 17.55 kJ of heat took place in a calorimeter and…

Q: As a lab experiment, a 10.0 g sample of iron metal, specific heat = 0.444 J/ g*oC, is heated from…

A: Mass of Fe = 10.0 g Mass of water = 50 g Initial temperature of Fe = 1600 °C Initial temperature of…

Question

2) The specific heat capacity of iron is 0.461 J/g K and 0.544 J/g K for titanium. A sample
consisting of a mixture of 10.0g Fe and 10.0g Ti at 100.0 °C loses 200 J of heat to the
environment. What is the final temperature of the sample?
a. 89.9 °C
b. 80.1 °C
c. 60.2 °C
d. 39.8 °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 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

The specific heat capacity of copper is 0.385 J g1 C1, whereas it is 0.128 J g1 C1 for gold. Assume you place 100. g of each metal, originally at 25 C, in a boiling water bath at 100 C. If energy is transferred to each metal at the same rate, determine which piece of metal will reach 100 C first.
How much will the temperature of a cup (180 g) of coffee at 95 C be reduced when a 45 g silver spoon (specific heat 0.24 J/g C) at 25 C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same density and specific heat as water.
A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J/C g) are heated to 100.0C. The mixture of hot iron and aluminum is then dropped into 97.3 g water at 22.0C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?
Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)
Hydrogen gives off 120. J/g of energy when burned in oxygen, and methane gives off 50. J/g under the same circumstances. If a mixture of 5.0 g hydrogen and 10. g methane is burned, and the heat released is transferred to 50.0 g water at 25.0C, what final temperature will be reached by the water?
A sample of 0.562 g of carbon is burned in oxygen in a bomb calorimeter, producing carbon dioxide. Assume both the reactants and products are under standard state conditions, and that the heat released is directly proportional to the enthalpy of combustion of graphite. The temperature of the calorimeter increases from 26.74 C to 27.93 C. What is the heat capacity of the calorimeter and its contents?
A 500.0-g sample of an element at 195C is dropped into an ice--water mixture; 109.5 g ice melts and an ice--water mixture remains. Calculate the specific heat of the element. See Exercise 131 for pertinent information.
Using the data in Appendix G, calculate the standard enthalpy change for each of the following reactions: (a) Si(s)+2F2(g)SiF4(g) (b) 2C(s)+2H2(g)+O2(g)CH3CO2H(l) (c) CH4(g)+N2(g)HCN(g)+NH3(g) ; (d) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)
You wish to heat water to make coffee. How much heat (in joules) must be used to raise the temperature of 0.180 kg of tap water (enough for one cup of coffee) from 30C to 96C (near the ideal brewing temperature)? Assume the specific heat is that of pure water, 4.18 J/(gC).
9.32 The material typically used to heat metal radiators is water. If a boiler generates water at 79.5°C, what mass of water was needed to provide the heat required in the previous problem? Water has a specific heat of 4.184Jg1 C1 .
The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

SEE MORE TEXTBOOKS