How many milliliters of water at 23 °C with a density of 1.00 g/mL must be mixed with 180 mL of coffee at 95 °C so that the resulting combination will have a temperature of 60 °C? Assume that coffee and water have the same density and the same specific heat (4.184 J/g°C). (write the answer without decimals)

How many milliliters of water at 23 °C with a density of 1.00 g/mL must be mixed with 180 mL of coffee at 95 °C so that the resulting combination will have a temperature of 60 °C? Assume that coffee and water have the same density and the same specific heat (4.184 J/g°C). (write the answer without decimals)

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

An unknown hot metal at 122.41°C with a mass of 53.37g was mixed with 28.15g of water at an initial temperature of 19.28°C. A final temperature (for both water and metal) of 22.27°C was reached. In units of J/(g°C), what is the specific heat of the unknown metal?
A 125 g piece of metal is heated to 288°C and dropped into 85 g of water at 12°C. The metal and water come to the same temperature of 24°C. What is the specific heat of the metal in joules over grams degrees Celsius?
A) An iron nail with a mass of 12 gg absorbs 15 J of heat. If the nail was initially at 30 ∘C, what is its final temperature? Express your answer using two significant figures. B) When 47.1 J of heat is added to 13.8 g of a liquid, its temperature rises by 1.74 ∘C. What is the heat capacity of the liquid?
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.80kg of water at 27.4°C . During the reaction 140.kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18J·g−1·K−1 . Be sure your answer has the correct number of significant digits.
What is the final temperature (in degrees Celsius) when 1940 J of energy are put into a 250 milliliter (mL) sample of water at 25.0 °C? The specific heat capacity of water is 4.184 J/g⋅°C. (Assume the density of water is 1.00 g/mL)
A 47.0-g sample of copper at 99.3 °C is dropped into a beaker containing 158 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g ⋅ K and 0.385 J/g ⋅ K, respectively.)
A 43.9 g spoon made of pure silver (c = 0.235 J/g C) at 20.1 celcius is used to stir an 8 oz. (240 g) cup of coffee at 9.12 celcius. what is the final temperature of the coffee? Assume that the coffee is an insulated container and the spoon absorbs all of the heat from the coffee, and that the coffee has the same specific heat as water.
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator it has a temperature of 175 °F. Calculate the amount of heat transferred from the engine to the surroundings by 10 grams of water with a specific heat of 4.184 J/g °C.
If 391.5 Joules of heat are added to 27.96 grams of a liquid, raising the temperature of the liquid from 29.6°C to 34.0°C, what is the specific heat capacity of the liquid with units of J/g•°C? Report your answer with 3 significant figures.
round to the correct number of significant digits
A 18g sample of a material absorbed 898 calories, raising the temperature of the anitmony from 33 degrees C to its melting point (389 degrees C). Calculate the specific heat (cal/g degrees C) of this material.
A 31.65 g piece of metal at 30.0 °C is placed in 50.0 g of water at 96.5 °C. The specific heat capacity of water is 4.184 J/gºC and that of the metal is 10.3 J/gºC. What is the final temperature in °C of the metal? Enter your answer using 1 decimal place and without unit.