A chemist carefully measures the amount of heat needed to raise the temperature of a 1.59 kg sample of a pure substance from -2.6 °C to 19.5 °C. The experiment shows that 24.9 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits.

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.59 kg sample of a pure substance from -2.6 °C to 19.5 °C. The experiment shows that 24.9 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 66AP

See similar textbooks

Similar questions

The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
A 5-mmdiameter hailstone has a terminal velocity of10.0m/s. Assuming its mass is6.031025 kg and all of its kinetic energy turns into heat, calculate the temperaturechangeof the hailstone when it hits the ground and stops. The heat capacity of ice is 2.06J/g.K.
In Example 3.5, a heat capacity of 20.78J/molK was used, which is 5/2R. Is this value of heat capacity justified? Why?
A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into 1.00 L deuterium oxide ("heavy water;" specific heat capacity = 4.21 I J/C g) at 25.5C. The final temperature of the uranium and deuterium oxide mixture is 28.5C. Given the densities of uranium (19.05 g/cm3) and deuterium oxide (1.11 g/mL). what is the edge length of the cube of uranium?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
at if Hess’s law were not true? What are some possible repercussions this would have?
Calculate the specific heat of a material if 288J of energy were required to heat 50.5g of the material from 298K to 330K. What are the units?
Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
Explain why the high-temperature reservoir of a heat engine must, indeed, be higher in temperature than the low-temperature reservoir. Can it ever be the other way around?
A piston reversibly and adiabatically contracts 3.88 moles of ideal gas to one-tenth of its original volume, thenexpands back to the original conditions. It does thisa total of five times. If the initial and final temperatures both are 27.5C, calculatea thetotal work andb thetotal U forthe overall process.