A 55.0 g sample of brass is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The brass sample starts off at 86.7 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 26.5 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to the correct number of significant digits. 0- g-°C X S thermometer- insulated container water sample. a calorimeter

A 55.0 g sample of brass is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The brass sample starts off at 86.7 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 26.5 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to the correct number of significant digits. 0- g-°C X S thermometer- insulated container water sample. a calorimeter

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...

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A 50.5 g sample of quartz is put into a calorimeter (see sketch at right) that contains 150.0 g of water. The quartz sample starts off at 98.8 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 19.5 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to 2 significant digits. J g. °C x10 X S thermometer. insulated container water sample a calorimeter ? ola
Consider two 50.0 mL volumes of water, one at 20.0 °C and the other at 100.0 °C. The temperature of the combined solutions when mixed in a calorimeter is measured to be 52.4 °C. What are the temperature changes for each of the volumes of water?
thermometer. insulated container A sample of quartz, which has a specific heat capacity of 0.730 J-goC, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 90.0 °C and the temperature of the water starts off at 25.0 °C. When the temperature of the water stops changing it's 27.1 °C. The pressure remains constant at 1 atm. water Calculate the mass of the quartz sample. Be sure your answer is rounded to 2 significant digits. 0 x10 X ? a sample a calorimeter do F
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.54 kg sample of C5H₁2S from 5.8 °C to 17.4 °C. The experiment shows that 3.51 × 104 J of heat are needed. What can the chemist report for the molar heat capacity of C5H₁2S? Be sure your answer has the correct number of significant digits. 12 - 1 – 1 K J. mol x10 X Ś 6 0 U
You have a sample of water with an unknown amount of mass. You add 348J of heat to the sample and measure the change in temperature to be increasing by 5.2 degrees celsius. What is the mass of the sample of water? The specific heat of water is 4.18 J/(g x degrees Celsius).
If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
A 54.5 g sample of brass is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The brass sample starts off at 95.8 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 16.4 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to 2 significant digits. П J g.°C x10 X S thermometer insulated container water sample a calorimeter U!!! 0 C
A 52.0 g sample of quartz is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 98.2 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 21.3 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to the correct number of significant digits. g.°C ? O
Can you explain where did I go wrong, I keep getting the same answer.
To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 15.2 g, and its initial temperature is −13.9 ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.9⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table. Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H 2 O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H 2 O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H 2 O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) *