Question

A 100g sample of each of the following metals is heated from 35C to 45C. Which...

A 100g sample of each of the following metals is heated from 35C to 45C. Which metal absorbs the highest amount of heat energy?

Copper- 0.385J/(g x C)

Magnesium- 1.02J/(g x C)

Mercury- 0.138J(g xC)

Silver- 0.237 J/(g x C)

Lead- 0.129 J/(g x C)

Homework Answers

Answer #1

q = msT

   = 100*0.385*10 = 385 J Copper

q = msT

   = 100*1.02*10 = 1020 J Magnesium

q = msT

   = 100*0.138*10 = 138 J Mercury

q = msT

   = 100*0.237*10 = 237 J Silver

q = msT

   = 100*0.129*10 = 129 J Lead

Magnesium absorbs the highest amount of energy.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. A 74.20 kg piece of copper metal is heated from 21.5°C to 335.1°C. Calculate the...
1. A 74.20 kg piece of copper metal is heated from 21.5°C to 335.1°C. Calculate the heat absorbed (in kJ) by the metal. 2. A sheet of gold weighing 10.9 g and at a temperature of 17.3°C is placed flat on a sheet of iron weighing 23.9 g and at a temperature of 52.2°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must...
Two samples of copper metal (20.0g and 100.0g) are heated using boliing water (T=100C). The 20.0g...
Two samples of copper metal (20.0g and 100.0g) are heated using boliing water (T=100C). The 20.0g sample is heated for 120 minutes white the 100.0g sample is heated for 60 minutes. Assuming it takes only 30 minutes for the metals to reach thermal equilibrium with the water regardless of the amount of metal, what can be said about the final temperature and energy content (the heat) of the metal samples?
The following table lists the specific heat capacities of select substances: Substance Specific heat capacity [J/(g⋅∘C)]...
The following table lists the specific heat capacities of select substances: Substance Specific heat capacity [J/(g⋅∘C)] silver 0.235, copper 0.385, iron 0.449, aluminum 0.903, ethanol 2.42, water 4.184, Water (2430 g ), is heated until it just begins to boil. If the water absorbs 5.07×105 J of heat in the process, what was the initial temperature of the water? Express your answer with the appropriate units.
Answer the following questions: a) A sample of lead with a mass of 1.45 kg is...
Answer the following questions: a) A sample of lead with a mass of 1.45 kg is heated until it reaches its melting point at 330 C. The lead is then heated further until it has entirely melted. During this process, the lead absorbs a total of 4.46 * 10 ^ 4 J as heat. What is the temperature at which the lead is initially heated? b) Gallium melts at 29.78 C, a temperature that can be achieved by the atmosphere...
19. How much heat is liberated (in kJ) from 2.47E+2 g of silver when it cools...
19. How much heat is liberated (in kJ) from 2.47E+2 g of silver when it cools from 8.86E+1 °C to 2.57E+1 °C? The heat capacity of silver is 0.235 J g^{-1} °C^{-1} g−1°C−1. Note, "heat liberated" implies that the change in heat is negative. Enter a positive number 20. A sample of sand initially at 2.18E+1 °C absorbs 1.386E+3 J of heat. The final temperature of the sand is 6.7E+1 °C. What is the mass (in g) of sand in...
An insulated container is used to hold 43.6 g of water at 20.6 °C. A sample...
An insulated container is used to hold 43.6 g of water at 20.6 °C. A sample of copper weighing 11.0 g is placed in a dry test tube and heated for 30 minutes in a boiling water bath at 100.0°C. The heated test tube is carefully removed from the water bath with laboratory tongs and inclined so that the copper slides into the water in the insulated container. Given that the specific heat of solid copper is 0.385 J/(g·°C), calculate...
For each, provide a.type of reaction, b. Molecular equation (balanced), c.Net ionic equation. 1. Mercury(II) oxide...
For each, provide a.type of reaction, b. Molecular equation (balanced), c.Net ionic equation. 1. Mercury(II) oxide and heat 2. Iron and oxygen (O2) 3. Water And sodium 4. potassium carbonate solution and calcium nitrate solution 5. silver nitrate solution and sodium chloride solution 6. Ammonium chloride solution and sodium sulfate solution 7. Potassium iodide solution and lead (II) nitrate solution 8. Sodium carbonate solution and hydrochloric acid 9. Potassium carbonate solution and acetic acid solution 10. Solid sodium bicarbonate and...
Problem 5.54 A 100.0-g bar of gold is heated from 25 ∘C to 50 ∘C during...
Problem 5.54 A 100.0-g bar of gold is heated from 25 ∘C to 50 ∘C during which it absorbs 322 J of heat. Assume the volume of the gold bar remains constant. Part A Based on the data, calculate the specific heat of Au(s). Express your answer to two significant figures and include the appropriate units. Cs = 0.13 J⋅(g⋅∘C)−1 SubmitMy AnswersGive Up All attempts used; correct answer displayed Part B Suppose that the same amount of heat is added...
Why does each metal ion have a different colored flame when heated? a. The amount of...
Why does each metal ion have a different colored flame when heated? a. The amount of energy released when an electron relaxes is different for each ion. b. The frequency of the electron is different depending on how hot the sample is heated. c. The amount of energy absorbed when an electron relaxes is different for each ion. d. The amount of energy released is different depending on how hot the sample is heated.
An 80.0-gram sample of a gas was heated from 25 °C to 225 °C. During this...
An 80.0-gram sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was done by the system and its internal energy increased by 6945 J. What is the specific heat of the gas?