3. Calculate the temperature change when:a) 10.0 kg of water loses 232 kJ of heat.10,0009=ATanxip)b) 1.96 kJ of heat are added to 500. g of copper.q=ATlylephaarhod 1300 joules SubstancewateraluminumcopperirongraniteSpecific Heat (J/g °C)4.1790.9000.3850.4500.790

The relationship between heat and temperature change is : => q =mc∆T where, q is the heat m is…

Answered: 3. Calculate the temperature change…

3. Calculate the temperature change when: a) 10.0 kg of water loses 232 kJ of heat. 10,000 9=DT (xep) b) 1.96 kJ of heat are added to 500. g of copper. q =AT (m) (EP)

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: the initial temperature of a 10.00 mL sample of water was 80o C and its final temperature is 21oC,…

Q: How many moles of CsHs (propane) must be reacted according to the following balanced chemical…

Q: How much would the temperature of 295 g of water increase if 17.4 kJ of heat were added? (the…

Q: What is the specific heat capacity of a substance if it takes 8.7 kJ of heat to warm 484.4 g by 39.1…

Q: A 10 g piece of copper at 145 oC is placed in 150 mL of water. The initial temperature of water is…

Q: C (s) + 02 (g) → CO2 (g) AH° = -393.5 kJ Calculate the heat change if 2.54 g of C is reacted.

A: The given reaction is: C(s)+O2(g)→CO2(g) ∆H°=-393.5 kJ Calculation of no. of mol of C: No. of…

Q: When 56 J of heat are added to 11 g of a liquid, its temperaturerises from 10.4oC to 12.7oC. What is…

A: Given that : Heat absorbed (q) = 56 J Mass of liquid = 11 g Temperature change (∆T) = 12.7°C -…

Q: Consider the followin thermochemical equation: 2NH3 (g) + 6H2O (g) -> 1/2 N2 (g) + 9H2 + 5/2 O2…

A: Reversing the equation-2:2NH3 (g) -> N2 (g) + 3H2 (g) ΔH° =+22.10 kcalReversing the equation-3…

Q: A 465 g iron ingot is taken from the furnace and immersed in 375 g of water in an insulated vessel,…

Q: If AH = -54.74 kJ for a chemical reaction, that reaction O is endothermic cannot occur is exothermic

A: In endothermic reaction heat is require while in exothermic reaction heat is given off.

Q: C (s) + 02 (g)- CO2 (g) AH° = -393.5 kJ Calculate the heat change if 2.54 g of C is reacted.

A: Given information, ∆H° ( for 1 mole of C(s)) = -393.5 kJ Mass of C(s) reacted = 2.54 g Molar mass of…

Q: In a calorimeter, a 90.0 g piece of metal at 92.4 *C is submerged in 100.0 g of water, that is…

A: In a calorimeter, a 90.0 g piece of metal at 92.4 °C is submerged in 100.0 g of water that is…

Q: How many litres of C6H14(I), measured at 20 C, must be burned to provide enough heat to warm 25.3 m3…

A: Given ,Objective :

Q: In a given gaseous reaction, 72 J of heat is absorbed and AE = -442 J. (a) Calculate w (work). work…

A: First law of thermodynamics When heat absorbed by a system Q=∆E+W Q=heat absorbed by a system…

Q: How much heat is released (negative value) if 19.955 g of a metal with heat capacity of 0.385 J/g°C…

A: The given mass of the metal (m) = 19.955 g Heat capacity of the given metal (C) = 0.385 J/g °C…

Q: 3 A backpacker collects snow at 0°C, and places it in a cooking pot on a camp stove. It takes 643 kJ…

A: It is given that: Total amount of heat (Q) = 643 kJ Specific heat capacity of water = 4.18 J/g.K…

Q: Calculate the quantity of energy needed to raise the temperature of 500mL EtOH from 0.00 (degrees)C…

A: Mass of ethanol = volume x density = 500 mL x 0.80 g /mL = 400 g.

Q: A home swimming pool contains 165 m3 of water. At the beginning of the swimming season, the water…

A: The amount of heat required is determined by using formula q= m c delta T

Q: A 39 g aluminum spoon (specific heat 0.904 J/g-°C) at 25°C is placed in 178 mL (177 g) of coffee at…

A: A definite quantity of heat is used up in raising temperature of substances. For substance that…

Q: Calculate the heat needed, in joules, to raise the temperature of 34 g iron, Fe, from 25oC to 78oC.…

A: The amount of heat absorbed (or released) by fixed amount of a substance to change its temperature…

Q: 20.0 g sample of aluminum (specific heat = 0.902 J g-1 C-1) with an initial temperature of 48.6C…

A: Given that: Mass of aluminium(m) = 20.0g Specific heat (C) = 0.902J/g°C Initial temperature(Ti) =…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.54 kg sample…

Q: When thermal energy is transferred from the system to its surroundings, heat (q) is:

A: When thermal energy is transferred from the system to its surroundings, heat (q) is negative It is…

Q: The Aq of a system that releases 12.4 J of heat to surroundings is O 12.4 J O -12.4 J Not enough…

A: The objective of the question is to determine the change in heat (Δq) of a system that releases 12.4…

Q: What is the change in temperature in deg. C of 24.5 g of ethyl alcohol that is heated with 310.2…

Q: 4. 448 Joules of heat are required to raise the temperature of a 10 gram sample of metal from 10…

Q: A piece of hot metal, X, weighs 24.50 g. After heating in a steam bath at 100.0oC, it is plunged…

A: The principle used here is Heat loss by metal = heat gained by water

Q: ,11) [References) Use the References to access important values if needed for this question. In the…

Q: When 156 g of water at a temperature of 22.5°C is mixed with 65.1 g of water at an unknown…

A: This is a question from mixing of substances.

Q: ystem does 675 kJ of energy onto its surroundings while releasing 1543 J of heat. What is the change…

A: To find the change in energy of the system, you need to consider both the work done by the system…

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

Q: Calculate the heat change in kilocalories for freezing 265 g of water at 0 degrees Celsius.

A: Mass of water = 265 g

Q: What mass of water will change its temperature by 3.00 degrees C when 525 J of heat is added to it?

A: The answer to the following question is-

Question

3. Calculate the temperature change when:
a) 10.0 kg of water loses 232 kJ of heat.
10,000
9=AT
anxip)
b) 1.96 kJ of heat are added to 500. g of copper.
q
=AT
lylep
haarhod 1300 joules

Substance
water
aluminum
copper
iron
granite
Specific Heat (J/g °C)
4.179
0.900
0.385
0.450
0.790

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: Explanation of formula

VIEW

Step 2: Calculation

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

A 25.0 g block of Al with specific heat 0.897 is placed into 100.0 g of water at 30.0°C. The final temperature of the system is 38.0°C What is the initial temperature of the Al? • Round your answer to the nearest ten. • Use 4.184 for the specific heat of water.
An electrical heater is used to supply 235.0 J of energy to a 15.0 g sample of water, originally at 295.0 K. Determine the final temperature in degrees Kelvin. (the specific heat capacity for water is 75.291 Jmol-1K-1)
Calculate the amount of coke, (carbon) needed to be burned in order to heat 500.kg of water from 20 degreees celsius to 50 degrees celsius. The heat of combustion of coke is 36.15 kj/g
A sample of sand initially at 2.24E1 °C absorbs 1.357E3 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}.
00 %24 0O р 9. %23 temperature? (Assume that no heat is lost to the surroundings; d of water is 1.00 g/mL.) 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
In a calorimeter, a 75.0 g piece of metal at 98.6 *C is submerged in 100.0 g of water, that is initially at 21.8 *C. When the metal and water reach thermal equilibrium, the temperature is 26.2 *C. What was the heat capacity of the metal (3 sig figs)?
The specific heat of certain type of cooking oil is 0.418 cal/(g.•C). How many heat energy is needed to raise to the temperature of 1.148 kg of this oil from 23.0 •C to 60.0•C?
You are performing an experiment where you place 9.2113 g of Al metal at 205.02 C into a coffee cup calorimeter that contains 98.4 g of water at 25.05 C. The final temperature of the water in the coffee cup is 28.89 C.Calculate the heat (q), in J, gained by the water using the equation, , given cwater= 4.184 J/g°CDo not include units. If you need to express your answer as an exponential number, use this template: 1445 should be typed as 1.445e+003
A block of copper(0.230+mol) starts at 15.5 degrees Celsius. What is the final temperature of cu if 226 cal of heat are added to it?
An 80.0g sample of metal, initially at 96 degrees C, is placed into 150g of water initially at 26 degrees C in a calorimeter. The final temperature of the water is 28.1 degrees C. What is the specific heat of the metal?
How many grams of an unknown substance, having a specific heat of 1.66 J g ° C, are present if a temperature change of -173.4 K occurs. The heat lost was 35981 J.