||| hochen stry Using specific heat capacity to find temperature change A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 5.40 kg of water at 22.3 °C. During the reaction 55.4 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 4.18 J.g¹.K¯¹. Round your - 1 answer to 3 significant digits. 11°C °℃ x10 1/5 × Ś Taylor Fol 6 0 E

||| hochen stry Using specific heat capacity to find temperature change A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 5.40 kg of water at 22.3 °C. During the reaction 55.4 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 4.18 J.g¹.K¯¹. Round your - 1 answer to 3 significant digits. 11°C °℃ x10 1/5 × Ś Taylor Fol 6 0 E

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

When 21.0 g of 0.200 M NaCl(aq) at 18.7 °C is added to 18.0 g of 0.100 M AgNO3(aq) at 18.7°C in a calorimeter, the temperature increases to 20.0 °C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g °C, what is the amount of heat in J produced?
1. In an experiment to determine the Specific Heat of Nickel, a 66.0 g sample of Nickel metal is heated to a temperature of 101.0 °C in a bath of boiling water. The Nickel is then removed from the Water bath and quickly added to a calorimeter containing 80.0 g of Water [C, of Water = 4.18 %g °cl at an initial temperature of 23.6 °C. After thermal equilibrium was reached, the final temperature of the system was 31.1 °C. a. What is the Specific Heat of Nickel, as determined by this experiment?
A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.51 kg sample of C,H,N from 44.7 °C to 57.9 °C. The experiment shows that 4.02 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,N? Round your answer to 3 significant digits. OJ-mol 1 - 1 ·K х10
A metal object with mass of 24.9 g is heated to 97.0 ∘C and then transferred to an insulated container containing 86.9 g of water at 20.5 ∘C.. The water temperature rises and the temperature of the metal object falls until they both reach the same final temperature of 24.1 ∘C. What is the specific heat of this metal object? Assume that all the heat lost by the metal object is absorbed by the water.
how to approach
A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 38.86°C. The specific heat capacity of water is 4.184 J g.°C and the density of water is g 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = = °C
A 2.59 g sample of a substance suspected of being pure gold (Cs = 0.128 J g−1°C−1) is warmed to 81.3 °C and submerged into 14.8 g of water initially at 24.0 °C. The final temperature of the water and the gold is 26.9 °C. Assume that the specific heat capacity of water is 4.18 J g−1°C−1.What is the heat capacity of the unknown substance? Express your answer to 3 significant figures.
O Thermochemistry = Using specific heat capacity to find temperature change 1/3 Bishop A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 8.70 kg of water at 33.2 °C. During the reaction 106. 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 4.18 J-g K. Round your answer to 3 significant digits. -1 C CP
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.19 kg sample of C,H,N from -4.5 °C to 6.6 °C. The experiment shows that 6.14 × 10° J of heat are needed. What can the chemist report for the molar heat capacity of C,H,N? Round your answer to 2 significant digits. O J-mol -1 - 1 ·K х10 ?
An experiment was performed to calculate the heat of solution for potassium fluoride. Use the following data to determine its heat of solution. Assume that the specific heat capacity of the solution produced is the same as that of water, 4.184 J⁄g·°C. Identity of Salt KF Mass of water in calorimeter (g) 52.42 Mass of salt sample (g) 7.32 Initial temperature of Calorimeter (°C) 20.8 Final temperature of Calorimeter (°C) 30.3 Report your answer in kJ/mol to 3 significant figures.
1. A certain two-step process involves transfer of heat and work between the system and the surroundings. In the first step, the internal energy, AE, of the system increases by 115.4 J when 95.1 J of work is done on the system. In the second step, the internal energy of the system decreases by 32.2 J when 15.6 J of work is done on the surroundings. In the first step of the two-step process, how much heat, in Joules, was absorbed or released? b. How much heat, in Joules, was absorbed or released in the whole two-step process? a.