A 45.00g sample of metal is heated to 98.0°C and placed in 100.00g of water at 21.0°C in a Styrofoam cup. The temperature of the water in the cup rises to 24.0°C as the metal cools. (a) Determine the specific heat of the metal. *

A 45.00g sample of metal is heated to 98.0°C and placed in 100.00g of water at 21.0°C in a Styrofoam cup. The temperature of the water in the cup rises to 24.0°C as the metal cools. (a) Determine the specific heat of the metal. *

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Energy

Section: Chapter Questions

Problem 26A

See similar textbooks

Related questions

Q: 4. An amount of heat equal to 2500 J is added to a system, and 1800 J of work is done on the system.…

Q: If you know that 18.5 grams of a particular mineral, with heat quantity of 1170 J, its temperature…

A: Hii There! since there are multiple question posted. we are answering first question. if you need…

Q: What is the change in internal energy

Q: A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample…

Q: What is the change of internal energy in J of a system that releases 675 J of heat and has 875 J of…

A: According to first law of thermodynamics, we have : dU = q + w ----(1) Where dU is change in…

Q: If a system absorbs 155.0 kJ of heat from its surroundings and the system does 65.0 kJ of work on…

A: Given that, System absorb heat, so q is positive, so, q=+155.0 KJ also given, system does work, so…

Q: If a system has 48 J of work done on it and absorbs 22 J of heat, what is the value of AE for this…

A: Given: Work done on the system (w) = +48 J Amount of heat absorbed = +22 J

Q: What is the change in internal energy for a system if the system absorbs 537 kJ of heat and does…

A: We have given that Heat absorbed by system =q= 537KJ Work done by system is always negative W =…

Q: A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample…

A: Using the following equation, the mass of the metal is calculated.

Q: How much heat must be applied to a 40.2g sample of gold (s=0.129 J(g∙℃)) in order to raise its…

A: Given information:Mass of gold = 40.2 gInitial temperature = 28.2 ˚CFinal temperature = 351.5…

Q: If a system absorbs 155.0 kJ of heat from its surroundings and the system does 45.0 kJ of work on…

A: Internal energy of a system is the overall energy that belongs to the system. Heat is denoted by…

Q: A system does 467 kJ of work and loses 157 kJ of heat to the surroundings. What is the change in…

A: First law of thermodynamics It states states that heat is a form of energy, and thermodynamic…

Q: A piece of silver with a mass 418 g has a heat capacity of 99.1 J/°C. What is the specific heat of…

A: Given, heat capcity 'c' of silver = 90.1 J/oC , mass of silver = 418 g, specific heat = ?

Q: A 52.7 g. piece of an unknown metal is heated up 51.4 °C when given 3492 J of heat. What is the…

A: Formula : Heat, q = msΔT 3492 = 52.7 x s x 51.4 s = 1.289 J g-1 °C-1 Here s is specific heat…

Q: If a system has 49.5 J of heat added to it, and the system does 75.5 J of work on its surroundings,…

A: According to the first law of thermodynamics, the relationship between work, heat and change in…

Q: Q1:- Find the external work done by the system in kcal, when 10 kcal of heat is supplied to the…

A: ✓The First Law of Thermodynamics states that heat is a form of energy, and thermodynamic processes…

Q: Suppose you heat a metal object with a mass of 30.0 g to 95.5 °C and transfer it to a calorimeter…

A: Given information is as follows: The mass of the metal = 30 g The initial temperature of the metal =…

Q: A gas does 135 J of work while expanding and, at the same time, absorbs 156 J of heat. What is its…

A: Given :- heat absorbed by system = 156 J work done by gas = 135 J To calculate :- ∆U(in J)

Q: What is the specific heat capacity of an unknown metal if 75.00 g of the metal absorbs 418.6J of…

A: Calculation of heat capacity: The amount of heat required to increase the temperature of one gram of…

Q: An experiment was conducted to determine the specific heat of platinum. It was determined that…

A: Heat required to raise the temperature = 158.8 Joules. Mass of a sample = 50.0 g Initial…

Q: A system releases 622 kJ of heat and does 105 kJ of work on the surroundings. What is the change in…

A: Internal energy is defined as the energy associated with the random, disordered motion of molecules.…

Q: If a system has 425 kcal of work done to it, and releases 5.00×102 kJ of heat into its surroundings,…

A: Convert the unit of work done to kJ:

Q: How much energy is needed to heat 180g of water from 28oC to 95oC? The specific heat of water is…

A: The amount of heat required to increases the temperature of the 1 g of the substance by 1 degree is…

Q: How much heat (in kJ) is required to raise the temperature of a 525.0 mL sample of water from 22.1 C…

A: The heat required to raise the temperature is directly proportional to the mass of sample and the…

Q: 1. A system receives 425 J of heat and delivers 425 J of work toits surroundings. What is the change…

A: We have to calculate the change of internal energy of system.

Q: The energy absorbed by a certain system is -130 kj . If the system does 90kj of work on the…

Q: If a system has 38.5 J of heat added to it, and the system does 75.5 J of work on its surroundings,…

A: According to the first law of thermodynamics,change in internal energy i.e∆U can be calculated by…

Q: If a system does 73.0 kJ of work on its surroundings and releases 105 kJ of heat, what is the change…

Q: A 192-gram piece of copper was heated to 100.0oC in a boiling water bath, and then it was dropped…

A: According to law of calorimetry heat absorbed = heat released. Copper has higher temperature so it…

Q: Calculate

A: The specific heat capacity of a substance is defined as the heat that is required to raise the…

Q: A18 kg block of iron at 29 °C is rapidly heated by a torch such that 11 kJ is transferred to it.…

Q: In a far planet from earth, a balloon containing a certain gas expands from 100 L to 250 L by…

Q: A hot lump of 37.0 g of copper at an initial temperature of 74.3 °C is placed in 50.0 mL H2O…

A: Given;

Q: A system suffers an increase in internal energy of 80 J and at the same time has 50 J of work done…

A: Given : Increase in internal energy ( U ) = +80 J Work done on the system ( W ) = +50 J Heat change…

Q: When 36 g of a metal at 89 C is added to 48 g of water at 27 C, the temperature of the water rises…

A: specific heat (Q) =m x S x ΔT MASS =m SPECIFIC HEAT =S CHANGE IN TEMPERATURE=ΔT

Q: If a system has 5.00 x 102 kcal of work done to it, and releases 5.00 x 102 kJ of heat into its…

Q: A 29.00 g sample of metal alloy is heated to 92.6 °C; then placed in 55.23 g of water in an…

Q: 4. A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample…

A: Please find your solution below :

Q: If a system does 84.0 kJ of work on its surroundings and releases 105 kJ of heat, what is the change…

A: According to FLT , Change in internal energy = Q + W

Q: If a system has 20.5 J of heat added to it, and the system does 75.5 J of work on its surroundings,…

A: Given: Heat consumed by the system is 20.5 J, and the work done by the system on the surrounding is…

Q: The air in an inflated balloon (defined as the system) warms over a toaster and absorbs 115 J of…

A: According to first law of thermodynamics, energy can neither be created nor destroyed, it can only…

Q: An experiment was conducted to determine the specific heat of platinum. It was determined that…

A: We have to calculate the specific heat (J/g°C) of platinum.

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.43 kg sample…

A: Given, mass of sample C4H11N, m = 0.43 kg Moles 0f C4H11N = 0.43 ×103 g73 g/mol change in…

Q: energylost by the Fewill be th the heat enérgy gained by- Mass of water 50.003 g Temperature of…

A: Given that :

Q: How much work is done on a system that the internal energy change of 105J and heat absorbed of 78J

A: From first Law of Thermodynamics , the total change in internal energy of the system can be…

Q: A 237 g sample of molybdenum metal is heated to 100.1 °C and then dropped into an insulated cup…

A: mass of Molybdenum = MMo = 237 gInitial Temperature of Molybdenum =TMo = 100.1°Cmass of water = Mw =…

Q: Iron bar of mass 869 g cools from 94 degree C to 5 degree C. Calculate the heat released by the…

A: Given : Mass of iron = 869 g Initial temperature of iron = 94 oC And final temperature of iron = 5…

Q: A metal radiator is made from 26.0 kg of iron. The specific heat of iron is 0.449 J g-1 °C-!. How…

A: Given : Mass of iron = 26.0 kg Specific heat = 0.449 J.g-1.°C-1 Initial temperature = 25.0°C…

Q: A gas expands and does 25.6 J of work on the surroundings. At the same time, the gas absorbs 89.6 J…

A: Solution W = 25.6J Since work is done by the system on the surrounding q = 89.6J Heat absorbed that…

Q: If a system absorbs 155.0 kJ of heat from its surroundings and the system does 95.0 kJ of work on…

Question

100%

A 45.00g sample of metal is heated to 98.0°C and placed in 100.00g of
water at 21.0°C in a Styrofoam cup. The temperature of the water in the
cup rises to 24.0°C as the metal cools. (a) Determine the specific heat of
the metal. *

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 1 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 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.
9.31 A metal radiator is made from 26.0 kg of iron. The specific heat of iron is 0.449Jg1C1 . How much heat must be supplied to the radiator to raise its temperature from 25.0 to 5 5.0°C?
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.
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.
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).
How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?
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?
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.
When calcium carbonate, CaCO3 (the major constituent of limestone and seashells), is heated, it decomposes to calcium oxide (quicklime). CaCO3(s)CaO(s)+CO2(g);H=177.9kJ How much heat is required to decompose 21.3 g of calcium carbonate?
Alloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the temperature ofthe alloy decreases by 106.1°C, while the temperature ofthe water increases by 10.5°C. What is the specific heat ofthe alloy?
9.82 The specific heat of gold is 0.13 J g-1 K-1 and that of copper is 0.39 J g-1 K-1. Suppose that we heat both a 25-g sample of gold and a 25-g sample of copper to 80C and then drop them into identical beakers containing 100 mL of cold water at 10°C. When each beaker reaches thermal equilibrium, which of the following will be true, and why? (You should not need to calculate the actual temperatures here.) (a) Both beakers will be at the same temperature. (b) The beaker with the copper sample in it will be at a higher temperature. (c) The beaker with the gold sample in it will be at a higher temperature