A house is built with a granite countertop. The heat capacity of the countertop is 151.8 kJC. A hot pan of water is placed on the countertop, and 6000 J of heat energy is transferred into the countertop. By how much does the temperature of the countertop change? °C 0.02516 AT = rect

A house is built with a granite countertop. The heat capacity of the countertop is 151.8 kJC. A hot pan of water is placed on the countertop, and 6000 J of heat energy is transferred into the countertop. By how much does the temperature of the countertop change? °C 0.02516 AT = rect

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 36E

See similar textbooks

Related questions

Q: A 113.25 gram sample of gold is initially at 100.0 °C. It gains 20.0 J of heat from its…

A: Heat formula will be used to calculate the final temperature of gold. Here it is: Heat = Mass of…

Q: When 762 joules of heat is added to a sample of solid copper (Cu), the temperature rises from 18.2…

A: We will use formula of heat

Q: A cook wants to heat 1.35 kg of water from 32.0oC to100.0 oC. If he uses the combustion of natural…

A: It is given that 1.35 kg of water will be heated from 32°C to 100°C using natural gas, which…

Q: In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a…

A: Interpretation- specific heat of aluminum Concept introduction- Specific heat- It is the amount of…

Q: heat in kJ

Q: You order a Grande (473 mL) pumpkin spice latte at Starbucks. It is too hot to drink (90. °C), so…

A: The following expression is used to determine the heat transferred from or to a substance. Q=mC∆T…

Q: Specific Heats of Substances Substance Specific Heat (J/g°C) Substance Specific Heat (J/g*C) Ice…

A: Answer

Q: A beaker contained 65.86 g of water at 18.41°C. A 85.03-g sample of metal at 68.95°C was placed in…

Q: It takes 54.0 J to raise the temperature of an 11.5 g piece of unknown metal from 13.0 Celcius to…

A: The relationship between heat required and specific heat of a substance is given below.

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 15.0 g piece of graphite is heated to 100.0 degrees C and placed in a calorimeter. The graphite…

A: The specific heat of graphite is calculated by using the following expression,

Q: A 125 g of metal is heated to 286 Celcius and dropped into 85.5g of water at 26.0 Celcius. The metal…

A: Heat Capacity: It may be defined as the amount of heat energy needed or loosen by anybody to change…

Q: A 15.0 g piece of graphite is heated to 100.0 degrees Celcius and placed in a calorimeter. The…

Q: A 167.8 g piece of iron initially at 25.0 Celsius, absorbs 10943 J of energy. What will the final…

Q: A 79-g piece of iron metal at 54.0 °C is placed in 29 g of water at 26.0 °C. Part A All the heat…

A: Given, mass of iron metal =79 ginitial temperature of iron =54.0°Cmass of water =26.0 °Cfinal…

Q: When 155 mL of water at 26°C is mixed with 75 mL of wa-ter at 85°C, what is the final…

A: The expression for the amount of heat transferred in the system is as follows,…

Q: Copper wires used to transport electrical current heat up because of the resistance in the wire. If…

Q: A 50.0-g sample of copper is at 25.0 degrees C. If 1 200 J of energy is added to it by heat, what is…

Q: repair crews to weld rails together. -) Ⓡ 2Fe(s) + Al2O3(s) DH rxn= -850 kJ -n, in grams, is formed…

A: Exothermic process is the one in which energy is liberated from the system to the surrounding in the…

Q: Calculate the specific heat of a 300.0g sample of iron. If it took 1000. Cal to raise the…

A: Mass of sample = 300 g Heat needed = 1000 cal ∆T = 123 oC

Q: In the laboratory a student finds that it takes 1Joules to increase the temperature of 13.3 grams of…

Q: Calculate the energy, in joules, to heat a cube of gold with a volume in of 12.0cm^3 from 15 Celsius…

Q: You pour a cup of tea that has a volume of 215.73 mL and is initially 91.06 °C. You place a silver…

A: Given , Volume of tea= 215.73 mL Initial temperature, Ti=91.06°C Specific heat of tea Ct= 4.186…

Q: A 25.64g sample of solid was heated in a test tube to 100 degrees Celcius in boiling water and…

A: Given:Mass of sample = 25.64gT = 100o CMass of water = 50 gTemperature increased from 25.10 degrees…

Q: A slab of iron ( 465g) is removed from an oven and plunged into 375g water in an insulated…

A: Given, Mass of iron, mi = 465gMass of water, mw = 375g(Tw)i = 26oC , (Tw)f = 87oC Cfe = 0.449 J/g oC…

Q: A glass contains 250.0 g of warm water at 78.0°C. A 50.0 g piece of gold at 2.30°C is placed in the…

Q: A beaker contained 64.74 g of water at 16.53°C. A 114.86-g sample of metal at 77.13°C was placed in…

Q: Suppose you heat a metal object with a mass of 30.1 g to 95.4 degrees celsius and transfer it to a…

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

Q: A mug is said to hold 66.05 g of water at 14.59°C. A 103.86-g spoon at 61.96°C was placed in it,…

Q: It takes 45.0 J to raise the temperature of an 11.8 g piece of unknown metal from 13.0∘C to 24.5 ∘C.…

A: The specific heat capacity for a given substance refers to the amount of heat that is needed to…

Q: heat in kJ

Q: A 125g piece of metal is heated to 288celcius and dropped into 85.0 g of water at 12.0 Celsius. The…

A: Given,Mass of metal = 125 gTemperature = 288 oCMass of water = 85.0 gTemperature = 12 oCFinal…

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: Calculate the heat capacity of a brick if 100. g sample absorbs 2439 J of heat, and it’s temperature…

Q: How much heat is required to raise the temperature of 6.21g sample of iron from 25.0 Celsius to 79.8…

A: Temperature change (ΔT) taking place in 6.21g of iron is given.

Q: 125g of zinc initially at 20 degrees celsius absorbs 500 J of heat, calculate the final temperature.

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: A 32 gram piece of metal is heated to a temeprature of 100 degrees celcius and placed into water.…

A: The relationship between heat ( q ) , specific heat ( s ) and change in temperature ( ∆T ) is q =…

Q: A piece of metal weighing 98.4 g with a specific heat of 0.46 Jg-¹ °C-1 at 1028.6 °C is dunked into…

A: Given that, The weight of the metal piece is mM = 98.4 g, The specific heat of the metal is CM =…

Q: The specific heat c of marble is 858 J/g K. How much heat is needed to heat 20 g of marble from 22…

A: Heat absorbed by the water bath is given by: q = m × C × ∆T Where, q = heat absorbed m = mass of the…

Q: It takes 45.0 J to raise the temperature of an 10.6 g piece of unknown metal from 13.0° C to 24.9…

A: Given :- Amount of heat absorbed = 45.0 J Mass of piece of metal = 10.6 g Initial temperature =…

Q: When 146.0 mL of water at 26.0°C is mixed with 41.0 mL of water at 85.0°C, what e fina temperature?…

A: given :- Volume of water at 26.0°C = 146.0 mL volume of water at 85.0°C = 41.0 mL To calculate :-…

Q: A 50.0 g piece of pure gold originally at 80.0°C is heated and in the process absorbs 100.0 J of…

A: Mass of gold=50.0g Energy absorbs= 100j C(gold)=0.129j/g°C T1= 80°C

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: How much energy is needed to raise the temperature of a 20.0g piece of copper from 15.0 degrees…

A: Specific heat capacity is defined as the quantity of heat absorbed by 1 gof substance to raise the…

Q: A beaker contained 65.15 g of water at 18.58°C. A 114.38-g sample of metal at 52.11°C was placed in…

Q: A cube of aluminum has a mass of 170 grams and its temperature rises from 15.0 °C to 21.0 °C when…

A: We can relate the quantity of a substance, the amount of heat transferred, its heat capacity, and…

Q: f we added 10,000 joules to gold at 20 degrees Celsius, its temperature would rise to 1570 degrees…

A: The heat absorbed by the gold metal can be expressed as follows: Q = mcTf - TiQ = Amount of heat…

Q: A glass contains 250.0 g of warm water at 78.0°C. A 50.0 g piece of gold at 2.30°C is placed in the…

Question

A house is built with a granite countertop. The heat capacity of the countertop is 151.8 KJC. A hot pan of water is placed on the
countertop, and 6000 J of heat energy is transferred into the countertop. By how much does the temperature of the
countertop change?
0.02516
AT =
correct
OCM

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 with 2 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

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.
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its volume decreases by 1.88 L. What is the change in internal energy of the gas?
A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5 C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.7 C. When thermal equilibrium is reached, the final temperature is 24.3 C. Calculate the specific heat capacity of titanium.
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 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?
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.
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?
A gas is cooled and loses 82 J of heat. The gas contracts as it cools, and work done on the system equal to 29 J is exchanged with the surroundings. What are q, w, and U?
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.
A 500-g sample of one of the substances listed in Table 7-1 was heated from 25.2C to 55.1C, requiring 133 J to do so. Which substance was it?
Three 45-g ice cubes at 0 C are dropped into 5.00 102 mL of tea to make iced tea. The tea was initially at 20.0 C; when thermal equilibrium was reached, the final temperature was 0 C. How much of the ice melted, and how much remained floating in the beverage? Assume the specific heat capacity of tea is the same as that of pure water.