he table shows the specific heat capacity of four substances. Heat Capacity Substance Aluminum 0.900 Glass 0.50 Carbon dioxide 0.843 Water 4.18 For an equal mass of each substance, which one will require the least amount of heat to raise its temperature from 20°C to 30°C? O Aluminum O Carbon dioxide Glass O Water O O O

he table shows the specific heat capacity of four substances. Heat Capacity Substance Aluminum 0.900 Glass 0.50 Carbon dioxide 0.843 Water 4.18 For an equal mass of each substance, which one will require the least amount of heat to raise its temperature from 20°C to 30°C? O Aluminum O Carbon dioxide Glass O Water O O O

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

Similar questions

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 90.0°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C. O 1.19 kg O 6.02 kg O 2.45 kg Ⓒ 3.30 kg O 7.94 kg
A chemist carefully measures the amount of heat needed to raise the temperature of a 203.0 g sample of a pure substance from -2.1 °C to 19.5 °C. The experiment shows that 609. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. 1 - 1 J.g¯¹.K x10 X Ś
A piece of unknown metal with a mass of 23.78 g is heated in boiling water to 97.4°C and then dropped into a coffee cup calorimeter containing 72.71 g of water at 13.65°C. When thermal equilibrium is reached, the final temperature is 24.79°C. Calculate the specific heat capacity of the unknown metal. The specific heat of water is 4.184 J/g/°C. Round your answer to 2 decimal places.
A chemist carefully measures the amount of heat needed to raise the temperature of a 165.0 g sample of a pure substance from -8.5 °C to 15.1 °C. The experiment shows that 541. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. 1 J.g .K - 1 x10 X 3
The specific heat of a certain type of metal is 0.149 J/g°C. What is the final temperature of 367 J of heat added to 74.3g of this metal, initially at 25.3°C?
Please don't provide handwriting solution
In an experiment, 26.5 g of metal was heated to 98.0°C and then quickly transferred to 150.0 g of water in a calorimeter. The initial temperature of the water was 22.5°C, and the final temperature after the addition of the metal was 32.5°C. Assume the calorimeter behaves ideally and does not absorb or release heat.
A 35.0 gram object has a specific heat of 0.832 Joules/gram °C. It gained 2095 Joules of heat from the surroundings. If it had started at 25.0 °C, what was the temperature of the object after it gained the heat from the surroundings? O 25.0 degrees Celsius O 3640 degrees Celsius O 71.9 degrees Celsius O 196.9 degrees Celsius O 1.74 degrees Celsius O 53.1 degrees Celsius O 96.9 degrees Celsius
A 325-g piece of gold at 427°C is dropped into 200.0 mL of water at 22.0°C. the specific heat of gold is 0.131 J/g°C. calculate the final temperature of the mixture. (assume no heat loss to the surroundings)
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.55 kg sample of a pure substance from 7.7 °C to 14.6 °C. The experiment shows that 5.5 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. DJ-g`1 - K-1 ☐ x10 X
6. If it takes 44.72 joules to heat a piece of metal weighing 16.89 g from 10.0°C to 29.0°C, what is the specific heat of the metal? op 19 0 no m f6 f7 0 f8
Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table. The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J J cal kJ 549 197 0.806