Given what you know about the specific heats of various substances, why are pots and pans made of metal? This is because they have low heat capacity; low specific heat O high heat capacity; high specific heat low heat capacity; high specific heat O high heat capacity; low specific heat

Given what you know about the specific heats of various substances, why are pots and pans made of metal? This is because they have low heat capacity; low specific heat O high heat capacity; high specific heat low heat capacity; high specific heat O high heat capacity; low specific heat

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 11P

See similar textbooks

Related questions

Q: How much energy as heat is required to raise the temperature of 50.00 mL of water from 25.04 °C to…

A: Given: Density of water at this temperature is 0.997 g/mL The specific heat capacity of liquid water…

Q: Adding 5.47 g of to 140 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt)…

A: According to the question, we are adding 5.47 g of NH4NO3 to 140 g of water in a coffee-cup…

Q: Àn aluminum (specific heat capacity = 0.90 Jig-*Č) calorimeter of mass 100 g contains 251 g of water…

A: Please find your solution below :

Q: A lead fishing weight with a mass of 57 g absorbs 146 calof heat. If its initial temperature is…

A: The given data contains, mass = 57 g. Heat Q = 146 cal. Initial temperature = 47°C

Q: A 30.14-g stainless steel ball bearing at 117.82°C is placed in a constant-pressure calorimeter…

A: In this process, the heat absorbed by the water is equal to heat release by the stainless steel…

Q: 5.37 A sheet of gold weighing 10.0 g and at a temperatureof 18.0°C is placed flat on a sheet of iron…

A: The heat lost from the iron sheet will be heat gained by the gold sheet as no heat is lost to the…

Q: A calorimeter contained 69.0 g of water at 15.99°C. A 119-g sample of iron at 66.26°C was placed in…

A: Initial temperature of calorimeter will be same as that of water . Heat capacity= mass × specific…

Q: In the laboratory a "cefee cup calerimer, or constant pressure calorimeter, in frequently und to…

A: Mass of Zn = MZn= 69.1 gInitial temperature of Zn = Tzn = 98.40°CMass of water = M = 82.88 gInitial…

Q: FR ön the surroundings heat and has work done on it by the surroundings heat and does work on the…

A: Internal energy(E) is the total energy of system. It can be changed by work and heat, ∆E = q + w To…

Q: 1. ransferred from one system to another spontaneously? What is heat? How does heat differ from…

Q: (a) What are the units of molar heat capacity? (b) What arethe units of specific heat? (c) If you…

A: (a) Molar Heat capacity is the heat required to raise the temperature of one mole of substance by…

Q: A gas is confined to a cylinder under constant atmosphericpressure, as illustrated in Figure 5.4.…

Q: An ideal gas in a cylinder fitted with a piston expands at constant temperature from a pressure of 9…

A: Given data : Temperature (T) = Constant Pressure (P) = 9 atm Volume(V) = 7.0 L to 17 LConsatnt…

Q: If a 68 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL of…

Q: A 31.55 g iron rod, initially at 22.7 °C, is submerged into an unknown mass of water at 63.2 °C, in…

Q: Iron pellets with total mass 17.0 g at a temperature of 92 °C are mixed in an insulated container…

Q: An unknown volume of water at 18.2oC is added to 24.4 mL of water at 35.0oC. If the final…

A: At 35o C water has a density of 1g/mL. Therefore, the mass of the warm water is, mass=density×volume…

Q: An unknown metal object is at 161C and placed into 3500 mL of cold water. If the metal object has a…

A: Given : Volume of water = 3500 mL Mass of metal = 2700 g Final temperature of metal = 35 oC Initial…

Q: If a 74.6 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL…

Q: In the construction of bridges andskyscrapers, gaps must be left between adjoining steel beams…

A: The given problem can be solved by using the formula given below as; q=m C ∆T…

Q: To make a pot of green tea, you must increase the mperature of the water 80°C. The pot contains 68g…

A: Specific heat capacity: The amount of heat required to raise the temperature of a unit mass of the…

Q: The specific heat capacity of benzene (C6H6) is 1.74J/g.K. How much energy is required to heat 168g…

A: Specific heat Specific heat of a substance is defied as the amount of the heat is used to increase…

Q: 12.755 g of a metal initially at 99.0ºC are placed into 75.0 g of water intially at 23.0ºC. The…

Q: Consider the following specific heats of metals.Metal Specific Heatcopper 0.385…

Q: An unknown organic compound is being proposed as an alternative to gasoline. The enthalpy of…

Q: Which Slatement is True? O a. The heat capacity of a substance does not depend on the amount of…

A: extensive properties are the properties which depends upon the amount of the substance , heat…

Q: A house is designed to have passive solar energy features.Brickwork incorporated into the interior…

Q: If 20.0 ml of 3.0 M HCl solution and 20.0 ml of 3.0 M NaOH solution at 215Care mixed in a…

A: Given data Volume of HCl = 20.0 mL Molarity of HCl = 3.0 M Volume of NaOH = 20.0 mL Molarity of…

Q: A piece of zinc at 20.0°C that weighs 60.0 g is droppedinto 200.0 g water at 100.0°C. The specific…

A: The final temperature reached by the zinc and the water has to be calculated,

Q: Two solid objects, A and B, are placed in boiling water and allowedto come to the temperature of the…

A: a). Larger heat capacity:

Q: How much heat? 3kg water, 0oC--> 100oC

A: We have :Mass of water = 3 kgInitial temperature = 0 °CFinal temperature = 100 °CSpecific heat of…

Q: An unknown organic compound is being proposed as an alternative to gasoline. The enthalpy of…

A: Heat of combustion of organic molecule = 0.391 g/mL It means 1 mL organic compound have = 0.391 g So…

Q: Three metal cylinders – one piece of iron, one piece of copper, and one piece ofaluminum – are…

A: Since heat capacity = specific heat capacity X mass Specific heat capacities of metal are (using…

Q: 45.0 g of copper (Cu) at -15.4 oC absorbed 613 J of heat and the final temperature is measured at…

Q: A 3.50-g sample of aluminum pellets (specific heat capacity - 0.89 JC-g) and a 21.50-g sample of…

Q: A layer of copper welded to the bottom of a skillet weighs 120 g. How much heat (in J) is needed to…

A: Relation between heat required (Q), specific heat capacity (c), mass (m) and temperature change (T2…

Q: A 328.00 sample of an unknown metal at 87.78°C is placed in a calorimeter containing 136.00 mL of…

A: The principle of the calorimeter is the heat energy transferred between the water in the calorimeter…

Q: A cubic piece of platinum metal (specific heat capacity = 0.1256 J/°C･g) at 200.0°C is dropped into…

A: Given: Specific heat capacity of platinum = 0.1256 J/ oC.g Temperature of platinum…

Q: A 32.6 g iron rod, initially at 22.7°C, is submerged into an unknown mass of water at 63.3 °C, in an…

Q: an a. Aluminum (specific heat capacity of 0.921 J/g°C) b. Copper (specific heat capacity of 0.377…

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

A: Here we are required to find the final temperature of water using the principle of calorimetry

Q: A calorimeter contained 79.0 g of water at 15.91°C. A 105-g sample of iron at 65.26°C was placed in…

A: Given data : Mass of iron = 105 g Mass of water = 79 g Final temperature of metal = 18.88°C…

Q: Metal A has a heat capacity of 0.450 J/g°C while metal B has a heat capacity of 1.250 J/g° C. If…

Q: If a material has a low heat capacity, the material will: OA cool slower than a material witha high…

A: The specific heat capacity of the material tells about the ability of a substance to retain the…

Q: 115 g of nickel at 150°C was placed in 1.0 kg of water at 27.1°C. Determine the final temperature of…

Q: A layer of copper welded to the bottom of a skillet weighs 171 g. How much heat (in J) is needed to…

A: The formula used is: Heat, Q = m× c×ΔT Where, m is mass, c is specific heat capacity and ΔT is…

Q: 9. Substance Mass (g) Initial Temperature(°C) AT (°C) Specific Heat Capacity (J/gx°C) Aluminum 20.0…

A: Given that, Mass of Al = 20.0 g Change in temperature ∆T = -5.9°C specific heat capacity of Al =…

Q: A 5.50-g sample of aluminum pellets (specific heat capacity = 0.89 J/°C·g) and a 18.00-g sample of…

Q: A cubic piece of platinum metal (specific heat capacity = 0.1256 J/°C･g) at 200.0°C is dropped into…

A: Solution- for the hreat trasfer process- heat lost by hot platinum = heat gained by deuterium…

Q: calculate heatE of a gas for a process in which the gas absorbs 25J of heat and does 7J of work by…

A: Consider the given information is as follows; Heat (q) = +25 J Work done by the system in expanding…

Question

Thanks!

Given what you know about the specific heats of various substances, why are pots and pans made
of metal?
This is because they have
low heat capacity; low specific heat
O high heat capacity; high specific heat
O low heat capacity; high specific heat
O high heat capacity; low specific heat

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

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

9.100 Two baking sheets are made of different metals. You purchase both and bake a dozen cookies on each sheet at the same time in your oven. You observe that after 9 minutes, the cookies on one sheet are slightly burned on the bottom, whereas those on the other sheet are fine. (You are curious and you vary the conditions so you know the result is not caused by the oven.) (a) How can you use this observation to infer something about the specific heat of the materials in the baking sheets? (b) What is themathematical reasoning (equation) that you need to support your conclusion?
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.
How many moles of isooctane must be burned to produce loo U of heat under standard state conditions?
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.
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
A piece of aluminum with a mass of 250. g is at an initial temperature of 5.0 C. If 24.1 kJ is supplied to warm the Al, calculate its final temperature. Obtain the specific heat capacity of Al from Table 4.1. Table 4.1 Representative Specific Heat Capacities
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
A7.50-gpiece of iron at 100.0C is dropped into 25.0g of water at 22.0C. Assuming that the heat lost by the iron equals the heat gained by the water,determine thefinal temperature of the iron/watersystem. Assume a heat capacity of water at 4.18 J/g.K and of iron at 0.452J/g.K.
What mass of carbon monoxide must be burned to produce 175 kJ of heat under standard state conditions?
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.