How much heat is liberated (in kJ) from 2.48E2 g of silver when it cools from 8.8E1 °C to 2.58E1 °C? The heat capacity of silver is0.235 Jg1°C-. Note, "heat liberated" implies that the change in heat is negative. Enter a positive number. A sample of sand initially at 2.19E1°C absorbs 1.379E3 J of heat. The final temperature of the sand is 6.7E1 °C. What is the mass (ing) of sand in the sample? The heat capacity of sand is 0.84 Jg-1°C-1.

Answered: Image /qna-images/answer/b1cbef84-b5a2-4c4f-b010-aa5e8240bd34.jpg

How much heat is liberated (in kJ) from 2.48E2 g of silver when it cools from 8.8E1 °C to 2.58E1 °C? The heat capacity of silver is 0.235 Jg-1°C-!. Note, "heat liberated" implies that the change in heat is negative. Enter a positive number.

How much heat is liberated (in kJ) from 2.48E2 g of silver when it cools from 8.8E1 °C to 2.58E1 °C? The heat capacity of silver is 0.235 Jg-1°C-!. Note, "heat liberated" implies that the change in heat is negative. Enter a positive number.

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: 15. Įmagine a glassblower drops 6.1 g of glass (specific heat capacity C:= 0.380 J/g.K) into 20.0 g…

Q: All of the heat from the combustion of 30.69 mL of C,H, is transferred to 7.513 L of water at…

A: 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) ΔHo = −6535 kJ Given, Volume of C6H6 = 30.69ml Density of…

Q: A hot lump of 35.6 g of aluminum at an initial temperature of 51.6 °C is placed in 50.0 mL H, O…

A: Mass of Aluminum = 35.6 g Initial temperature of Aluminum = 51.6°C Specific heat capacity = 0.903…

Q: 11. An electric motor produces energy to turn a fan blade. The energy used to turn the fan blade is…

A: Answer

Q: If 1.42 kcal of energy is required to raise the temperature of a 190 g sample of pure iron, by how…

A: Q - heat = 1.42 Kcal m - mass = 190 g C - specific heat =0.45 J/g-°C ΔT - change/rise in temperature…

Q: A chemical reaction in a bomb calorimeter produces 5.17 kJ of heat. If the heat capacity of the…

Q: piece of metal with a mass of 20.8 g is heated to 99.5°C and then dropped into an ideal "no-leak"…

A: Given that: Mass of metal(m) = 20.8g Initial temperature of metal(T1) = 99.5°C Mass of water(m) =…

Q: Given that iron has a specific heat capacity of 0.4490 J/g･°C, calculate the amount of heat (J) to…

A: The objective of this question is to calculate the amount of heat required to raise the temperature…

Q: Calculate the energy required to heat 367.0 g of aluminum from –3.6 °C to 13.2 °C. Assume the…

Q: A 5.00-g sample of liquid water at 25.0 °C is heated by the addition of 84.0 J of energy. T

Q: An automobile engine provides 621 Joules of work to push the pistons. In this process the internal…

A: According to the first law of thermodynamics, the following expression is obtained: ∆U=q+w…

Q: Part C at A piece of metal weighing 5.50 g at a temperature of 47.8 °C was placed in a calorimeter…

Q: mass

Q: Calculate the final temperature of the water after 2.47g of zinc at 60.1 C is added to 29.4g of…

Q: Calculate the energy required to heat 2.00 kg of silver from -6.1 °C to 10.2 °C. Assume the specific…

Q: A 818 g sample of metal with a specific heat capacity of 0.251 of J/g•ºC is initially at a…

A: Given Mass = 818 g Heat = 1.5 kJ = 1500 J T1 = 22.6°C Specific heat = 0.251 J/g-°C

Q: A 57-g sample of liquid water at 25.0 C is mixed with 21 g of water at 45.0°C. The final temperature…

A: We have to calculate the final temperature of water.

Q: 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature ( °C) if…

Q: A chemist measures the energy change AH during the following reaction: Cl₂(g)+H₂(g) → 2 HCl(g) ΔΗ=…

Q: Calculate the energy required to heat 1.30 kg of ethanol from -1.7 °C to 11.4 °C. Assume the…

A: Heat absorbed by the ethanol is given by:Where,q = heat absorbedm = mass of the ethanolCv = heat…

Q: A 2.62E1 g sample of aluminum at 1.008E2 °C is added to 1.002E2 g of water at 2.22E1 °C in a…

A: For a chemical reaction or physical process to occur a certain amount of energy should be furnished…

Q: The final temperature of the copper is ________°C.

A: q = mc∆T q is the amount of heat energy required m is the mass of substance c is the specific…

Q: Calculate the energy required to heat 133.0 mg of silver from -6.9 °C to 17.7 °C. Assume the…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Q: 9. What mass of natural gas (CH4) must burn to emit 3,447 kJ of heat? CH4 (g) + 202 (g) → CO2 (g) +…

A: The mass of CH4 can be calculated as follows

Q: A 350.0 g lead rod is heated and then is placed into an insulated vessel containing 50.0 g of water…

A: We know that if two bodies that have significant difference in temperature, are in contact, the heat…

Q: SLVER Massof EMPTY cup 4g Mass of cuptwater 64.0g Mass of waterR 64.0g 4.0g 60g Massof SILVER 260g…

Q: A gas expands and does work on the surroundings equal to 0.21 L atm. At the same time, it absorbs…

A: The question is based on the concept of chemical thermodynamics. We have to calculate internal…

Q: Which of the following statements is always true? A Solids have a larger heat capacity than liquids.…

A: Heat capacity= Q/m.∆T

Q: 1 Calculate the amount of heat needed to raise the temperature of 50.0 g of iron from 21.0°C to…

A: As per bartleyby guidelines i answered only first question so please don't mind and post other…

Q: A 54.12 g sample of a substance is initially at 25.4 °C. After absorbing 1603 J of heat, the…

A: We know that, Q = mc∆T Where, Q = heat m = mass c = specific heat ∆T = change in temperature

Q: The specific heat if a certain type of metal is 0.128 J/(g.C). What is the final temperature if 305…

A: Amount of heat,Q required to change the temperature of a substance of mass ,m and specific heat…

Q: Calculate the energy required to heat 430.0 mg of iron from -2.1 °C to 12.1 °C. Assume the specific…

Q: A 981.8 g sample of bismuth goes through a temperature change of +46.75 °C while absorbing 784.6…

A: 1. Given :- Mass of sample of Bi = 981.8 g Temperature change i.e. ∆T = +46.75°C Amount of heat…

Q: A 25.0g sample of copper at 25.0°Cis placed in 100.0 g of water at 40.0°C. The copper and water…

Q: All of the heat from the combustion of 39.10 mL of C,H, is transferred to 5.175 L of water at…

A: Given values: Volume of C6H6 is 39.10 mL Volume of water is 5.175 L. Initial temperature is 26.9°C.…

Q: A 42.32 g sample of a substance is initially at 21.3 °C. After absorbing 2983 J of heat, the…

Q: A 52.03 g sample of a substance is initially at 28.5 °C. After absorbing 1165 J of heat, the…

Q: 4.Determine the specific heat capacity of titanium if a 43.5 g sample absorbs 0.476 kJ (476J) as its…

A: Mass of titanium=43.5 gram Absorbed energy=0.47 6KJ=476J Temperature change=32°C-53°C

Q: The specific heat of a certain type of metal is 0.128 J/(g-°C). What is the final temperature if 305…

Q: A metal weighing 45.6g loses 350.6J of heat when it’s temperature is lowered from 89.2oC to 64.2o…

Q: The temperature of an 6.95 g sample of an unknown metal increases from 22.0°C to 31.7°C upon the…

A: The mass of the sample is = 6.95 g Increase in the temperature is = 22.0oC to 31.7oC The required…

Q: A chemist measures the energy change AH during the following reaction: Cl₂(g) + H₂(g) → 2 HCl(g) Use…

A: An EXOTHERMIC thermochemical reaction equation is written as Reactants ------> products + HeatOr…

Q: Calculate the energy required to heat 157.0 g of graphite from 4.3 °C to 13.8 °C. Assume the…

A: given mass of graphite = 157 g initial temperature = 4.3°C final temperature = 13.8°C specific heat…

Q: Calculate the energy required to heat 249.0 g of aluminum from -3.2 °C to 6.9 °C. Assume the…

A: • The values provided in the question are:- i) Mass of aluminium, m = 249.0 g ii) Initial…

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…

Question

How much heat is liberated (in kJ) from 2.48E2 g of silver when it cools from 8.8E1 °C to 2.58E1 °C? The heat capacity of silver is
0.235 Jg1°C-. Note, "heat liberated" implies that the change in heat is negative. Enter a positive number.

A sample of sand initially at 2.19E1°C absorbs 1.379E3 J of heat. The final temperature of the sand is 6.7E1 °C. What is the mass (in
g) of sand in the sample? The heat capacity of sand is 0.84 Jg-1°C-1.

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

#18
Perform the following heat calculation. show all work and include units on answer How much heat is required to raise the temperature of 10.0 g of iron from 25°C to 100.°C? The specific heat capacity of iron is 0.46 J/g°C
A system undergoes a process consisting of the following two steps:Step 1: The system absorbs 72 Jof heat while 35 J of work is done on it.Step 2: The system absorbs 35 J of heat while performing 27J of work.Assuming that the heat capacity of the system is 23 J/C and the initial temperatureis 25 C, calculate the final temperaturefor the overall process.
25.0 g of mercury is heated from 25 degrees celsius to 155 degrees celsius and absorbs 455 joules of what in the process. Calculate the specific heat capacity of mercury.
17.0 J of heat is added to 10.00 g of gold, which is initially at 25°C.The heat capacity of gold is 25.41 J/(mol • °C). What would be the final temperature of the gold?
A 79.1 g sample of an unknown solid is heated to 62.6ºC and placed into a calorimeter containing 92.1 g of water at 22ºC. If the final temperature of the solid sample and the water is 32.5ºC, what is the specific heat of the solid? Please provide your final answer rounded to two decimal places.
1. How many joules of energy would be required to raise the temperature of 3.2 grams of mercury 4.2°C? The specific heat of mercury is 0.14 J/(g.°C).
A 0.491 kg sample of an unknown metal loses 4.08 kJ of heat. If the change in its temperature was 22.4°C, calculate the specific heat capacity of the J metal in units if g°C
According to the following thermochemical equation, what mass of C3H18 (in g) must react in order to produce 345 kJ of energy? Assume excess O2. The molar mass of octane (C3H18 ) is 114.33 g/mol. 2 C3H18 + 25 O2 - 16 CO2 + 18 H2O AH°rxn = -11018 kJ Units don't need to be typed in the answer. Answer:
A 46-g sample of liquid water at 25.0 C is mixed with 22 g of water at 45.0°C. The final temperature of the water is ________°C. The specific heat capacity of liquid water is 4.18 J/g-K.
15.0 J of heat is added to 10.00 g of gold, which is initially at 25°C.The heat capacity of gold is 25.41 J/(mol • °C). What would be the final temperature of the gold?
A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.226 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C.