1A 22.0 g sample of iron, which has a specific heat capacity of 0.449 J.g °℃ is dropped into an insulated container containing 200.0 g of water at 65.0 °Cand a constant pressure of 1 atm. The initial temperature of the iron is 9.6 °C.IAssuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3significant digits.°Cx101X

mass of iron = 22.0 gspecific heat(c) of iron = 0.449 J/goCmass of water = 200.0 gspecific heat(c)…

A 22.0 g sample of iron, which has a specific heat capacity of 0.449 J.g¹.C-¹, is dropped into an insulated container containing 200.0 g of water at 65.0 °C and a constant pressure of 1 atm. The initial temperature of the iron is 9.6 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. °C x10 X 3

A 22.0 g sample of iron, which has a specific heat capacity of 0.449 J.g¹.C-¹, is dropped into an insulated container containing 200.0 g of water at 65.0 °C and a constant pressure of 1 atm. The initial temperature of the iron is 9.6 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. °C x10 X 3

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 56.2 g sample of aluminum, which has a specific heat capacity of 0.897 J-g¹C¹, is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the aluminum sample. Be sure your answer is rounded to the correct number of significant digits. °C X Ś thermometer- insulated. container water sample a calorimeter
A 20.0 g sample of polyisoprene, which has a specific heat capacity of 1.880 J-gc, is dropped into an insulated container containing 150.0 g of water at 30.0 °C and a constant pressure of 1 atm. The initial temperature of the polyisoprene is 94.2 "C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has the correct number of significant digits. C 2
A constant pressure calorimeter contains 286 g of water at 20.0 °C. A 13.41 g of substance X (molar mass 154 g/mol) at 20.0°C was dissolved in this water. The temperature of the solution increased to 23.5 °C. Assuming the specific heat of the mixture is 4.184 J g‑1°C‑1, and the density of the solution is 1.00 g/cm3, calculate the enthalpy change (in kJ) for the dissolution of 1 mole of X.
A 20.0 g sample of brass, which has a specific heat capacity of 0.375 J.g¹°C¹, is dropped into an insulated container containing 250.0 g of water at 75.0 °C and a constant pressure of 1 atm. The initial temperature of the brass is 9.0 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. °C x10 1 X Ś
1 " A 47.0 g sample of aluminum, which has a specific heat capacity of 0.897 J.g •°C is dropped into an insulated container containing 150.0 g of water at 20.0 °C and a constant pressure of 1 atm. The initial temperature of the aluminum is 95.0 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. °C x10 X
A sample of iron, which has a specific heat capacity of 0.449 J-g¹C¹, is put into a calorimeter (see sketch at right) that contains 150.0 g of water. The iron sample starts off at 85.1 °C and the temperature of the water starts off at 22.0 °C. When the temperature of the water stops changing it's 24.3 °C. The pressure remains constant at 1 atm. Calculate the mass of the iron sample. Be sure your answer is rounded to 2 significant digits. 08 X S thermometer. insulated container water- sample a calorimeter 區 de
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6334 g sample of acetylsalicylic acid (C9H8O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.100×103 g of water. During the combustion the temperature increases from 22.68 to 25.23 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 929.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of acetylsalicylic acid based on these data. C9H8O4(s) + 9O2(g) 4 H2O(l) + 9 CO2(g) + EnergyMolar Heat of Combustion = how many kJ/mol
A 48.0 g sample of glass, which has a specific heat capacity of 0.670 J.g ¹.°C¯¹, is dropped into an insulated container containing 200.0 g of water at 15.0 and a constant pressure of 1 atm. The initial temperature of the glass is 86.5 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has the correct number of significant digits. 17.63 °C x10 X Be Careful Please check the number of significant digits in your answer. OK
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 bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.1250 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.200×103 g of water. During the combustion the temperature increases from 23.58 to 26.40 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 979.8 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.C6H12O6(s) + 6O2(g) 6 H2O(l) + 6 CO2(g) + Energy
A sample of iron, which has a specific heat capacity of 0.449 J.g¹.°C¹, is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The iron sample starts off at 98.2 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 27.4 °C. The pressure remains constant at 1 atm. Calculate the mass of the iron sample. Be sure your answer is rounded to 2 significant digits. 1 g x10 X 5 thermometer. insulated container water sample a calorimeter
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol