Part A A volume of 75.0 mL of H20 is initially at room temperature (22.00 °C). A chilled steel rod at 2.00 °C is placed in the water. If the final temperature of the system is 21.40 °C, what is the mass of the steel bar? Use the following values: specific heat of water = 4.18 J/(g. °C) specific heat of steel = 0.452 J/(g- °C) Express your answer to three significant figures and include the appropriate units. > View Available Hint(s)

Part A A volume of 75.0 mL of H20 is initially at room temperature (22.00 °C). A chilled steel rod at 2.00 °C is placed in the water. If the final temperature of the system is 21.40 °C, what is the mass of the steel bar? Use the following values: specific heat of water = 4.18 J/(g. °C) specific heat of steel = 0.452 J/(g- °C) Express your answer to three significant figures and include the appropriate units. > View Available Hint(s)

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 821 g copper pan is removed from the stove at a temperature of 150 °C. It is then stacked on top of a 711 g aluminum sheet at room temperature, 25 °C. The specific heat capacity for copper is 0.387 and that for aluminum is 0.904 g-K Assume no heat g-K is gained or lost to the surroundings. What is the final temperature (T;) of the two objects after thermal equilibrium is reached? Tf = °C
If a 136.51 g Al rod (c = 0.900 J/g°C) is at 100.0°C and placed into 250.0 g of water at 21.8°C, what is the temperature of the system (rod + water) at equilibrium assuming %3D no losses to the surroundings? Assume the specific heat of water to be 4.18 J/g°C. (A 46°C 30°C c) 206°C 18°C
Calculate the total enthalpy change (kJ) for the following reaction: H2O (s, 90 g, –10. oC) --> H2O (l, 90 g, 10. oC) (The specific heat capacity of ice is 2.0 J/g×oC; the specific heat capacity of liquid water is 4.2 J/g×oC; the enthalpy of fusion for H2O at 0 oC is 6.0 kJ/mol.)
300.00 mL of 0.200 M aqueous KOH neutralizes 150.00 mL of aqueous 0.200 M H2SO4. If the initial temperature is 22.3 C and it rises to 29.2 C determine the molar heat fro the neutralization of KOH. Express your answer kj/mole KOH. The specific heat of solution is 4.190 J/g C. Assume the density of the solution is 1.00 g/mL
The first step in the industrial recovery of zinc from zinc sulfide ore is roasting, that is , the conversion of ZnS to ZnO by heating: 2ZnS(s) + 3O2(g) ⟶⟶ 2ZnO(s) + 2SO2(g) ΔH = -879 kJ/mol Calculate the heat evolved (in kJ) per gram of ZnS roasted. Group of answer choices 879 kJ 4.51 kJ 293 kJ 440 kJ 9.02 kJ
The thermite reaction, used for welding iron, is the reaction of FegO4 with Al. 8 Al (s) + 3 Fe3O4 (s) > 4 Al203 (s) + 9 Fe (s) AH° = -3350 kJ Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000°C. How much heat (in kJ) is released by the reaction of 16.5 g of Al with 76.7 g of Fe304? Enter your numerical answer in units of kJ.
Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction: 2Al(s) + Fe203(s) → Al203(s) + 2Fe(s) This reaction occurs when a mixture of powdered aluminum and iron(III) oxide is ignited with a magnesium fuse. The following enthalpies of formation are known: AH°; for Fe203(s) = -826 kJ AH°; for Al203(s) = -1676 kJ O 1251 kJ O 2502 kJ O-1251 kJ O 425 kJ 850 kJ O- 2502 kJ -850 kJ -425 kJ
Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.
Which of the following reactions occuring at 25° C defines the standard enthalpy of formation (TriangleHf) of liquid water? - 2 H (g) + O (g) -> H2O (l) - H2O(g) + O (g) -> H2O (l) - H2 (g) + ½O2 (g) -> H2O (l) - 2 H2 (g) + O2 (g) -> 2 H2O (l)
Per x M Inb x 31799#/7231799/2/0 ted 13 out of 16 16 P11 Essentials of General, Organic, and Biochemistry Denise Guinn THIRD EDITION The table lists the specific heat values for brick, ethanol, and wood. Specific Heats of Substances Substance Brick Ethanol Wood heat added: P S per: X 20 effe x CDC He: X JA 6 Specific Heat 0.20 0.58 0.10 B 10 X 4 gºC Calculate the amount of heat, in calories, that must be added to warm 96.8 g of brick from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. W 4 Calculate the amount of heat, in calories, that must be added to warm 96.8 g of ethanol from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. ○바 8 No X 9 EC eth X 0 Sm X 00 39 HR MIN SEC 0/R Sm x Resources + presented by Macmillan Learning G ا ا ا 200 L Next Qu cal 40 1
0.1 mole of liquid ethanol C;H;OH was burned in a bomb calorimeter with a heat capacity of 27.34 kJ.K. The temperature of the calorimeter was increased from 21.4°C to 26.4°C. a) Calculate the standard enthalpy change of combustion in kJ/mol. b) Calculate the standard enthalpy of formation for liquid C;H;OH in kJ/mol. c) For ethanol, AvapH° = 43.5 kJ/mol. Calculate q, w, AH and AU when 1.75 mole C;H;OH (I) is vaporized at 260 K and 765 Torr. AH° / kJ.mol H20(g) H20(1) CO2(g) -241.82 -285.83 -393.51 Suppose you have 1 mole of a monatomic ideal propane (C3H3) at 1 bar and 300 K. Calculate q, w, AH and AU for each of the processes described in part a, b, and c. a) The system undergoes a reversible isothermal expansion until its volume is tripled. b) The system undergoes an irreversible expansion until its volume is tripled and against an external pressure of 0.1 bar. c) The system undergoes a reversible process in which 1 kJ of heat is absorbed by the gas and the enthalpy change is -1.50…
A volume of 110. mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water. If the final temperature of the system is 21.50 ∘C , what is the mass of the steel bar? Use the following values: specific heat of water = 4.18 J/(g⋅∘C) specific heat of steel = 0.452 J/(g⋅∘C) Express your answer to three significant figures and include the appropriate units. View Available Hint(s) mass of the steel = nothingnothing Submit Part B The specific heat of water is 4.18 J/(g⋅∘C). Calculate the molar heat capacity of water. Express your answer to three significant figures and include the appropriate units.