A piece of unknown substance weighs 55.8 g and requires 1910 J to increase its temperature from 21.7°C to 87.4°C. (a) What is the specific heat (in J/g-°C) of the substance? 4.0 J/g.°C (b) If it is one of the substances found in the table below, what is its likely identity? Specific Heats of Common Substances at 25°C and 1 bar Substance Symbol (state) Specific Heat (J/g-°C) O gold Au(s) 0.129 O copper Cu(s) 0.384 O iron Fe(s) 0.449 O argon Ar(g) 0.521 O silicon Si(s) 0.712 O carbon dioxide Co,(0) 0.843 O aluminum Al(s) 0.904 O nitrogen N2(g) 1.039 water H20(1) 4.1801 O helium He(g) 5.196 Type here to search hp 112 fs f6 144 sc & 8 Q E A J K B. FL %24

A piece of unknown substance weighs 55.8 g and requires 1910 J to increase its temperature from 21.7°C to 87.4°C. (a) What is the specific heat (in J/g-°C) of the substance? 4.0 J/g.°C (b) If it is one of the substances found in the table below, what is its likely identity? Specific Heats of Common Substances at 25°C and 1 bar Substance Symbol (state) Specific Heat (J/g-°C) O gold Au(s) 0.129 O copper Cu(s) 0.384 O iron Fe(s) 0.449 O argon Ar(g) 0.521 O silicon Si(s) 0.712 O carbon dioxide Co,(0) 0.843 O aluminum Al(s) 0.904 O nitrogen N2(g) 1.039 water H20(1) 4.1801 O helium He(g) 5.196 Type here to search hp 112 fs f6 144 sc & 8 Q E A J K B. FL %24

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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The specific heat of a certain type of metal is 0.128 J/(g⋅∘C).0.128 J/(g⋅∘C). What is the final temperature if 305 J305 J of heat is added to 30.3 g30.3 g of this metal, initially at 20.0 ∘C?20.0⁢ ∘C? ?final=Tfinal= ∘C
When a chemist burns ammonia according to the reaction below she finds that the reaction releases heat. (It is exothermic.) 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) The enthalpy of the reaction DH = -1267 kJ. What is the enthalpy change (in kJ) when 3 grams of ammonia are burned?
A new substance evolves (-1.64) kJ of heat when 17.15 g it cools from 106.2oC to 23.8oC. What is the specific heat (in J/(g K)) of this substance?
Volume of cool water (mL) Volume of hot water (mL) Initial temperature of cool water (°C) Initial temperature of hot water (°C) Final temperature of water in calorimeter (°C) Temperature change for cool water (°C) Temperature change for calorimeter (°C) Temperature change for hot water (°C) Heat change for cool water (J) Heat change for hot water Heat change for calorimeter (J) Heat capacity of calorimeter (J/°C) Trial 1 50.0 47.5 24.3 38.9 37.0 Trial 2 50.0 46.1 24.9 35.0 33.7 Trial 3 50.0 44.8 23.3 33.8 30.8
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F2 (see the table). Specific Heats for Some Substances Substance Elements Aluminuim, Al(s) Copper, Cu(s) Gold, Au(s) Iron, Fe(s) Silver, Ag(s) Titanium, Ti(s) Compounds Ammonia, NH3(g) Ethanol, C₂H5OH(1) Sodium chloride, NaCl(s) Water, H₂O(1) Water, H₂O(s) 3 $ L cal/g °C J/g °C 0.214 0.897 0.0920 0.385 0.0308 0.129 0.108 0.452 0.0562 0.235 0.125 0.523 0.488 2.04 0.588 2.46 0.207 0.864 1.00 4.184 0.485 2.03 % 5 E R T Q Search F6 D F G F7 ▼ Part G Y Submit Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissio GH the energy lost when 18.3 g of gold cools from 224 °C to 113 °C 7 |Ε| ΑΣΦ Submit Part H ASUS Request Answer F8 Request Answer P Pearson J FO ? F10 J F12 Pu
When 40 g of a metal at 85 ◦C is added to48 g of water at 23 ◦C, the temperature of thewater rises to 29 ◦C. What is the specific heatcapacity of the metal? Assume no heat waslost to the surroundings.Answer in units of J/g · ◦C
Consider the reaction of ammonia gas with O2(g) according to the thermochemical equation given below: 4NH3(g) + 7O2(g) 4NO2(g) + 6H2O(1) AH° = -1132 kJ/mole (c) Write the thermochemical equation representing the combustion of 1 mole of ammonia. (d) Write the thermochemical equation representing the reaction of 1 mole NO2(g) with Hz0
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CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = ____kJ(c) If the enthalpy change is 18.0 kJ, how many grams of hydrogen gas are produced?____g(d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = ____kJ(e) Calculate E when 750.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K _____kJ HopHelpCh5N1
A silver kettle weighs 1.02 kg. (The specific heat of silver is 0.235 J/g·°C) (a) What is the heat capacity (in J/°C) of the kettle? _______________ J/°C (b) How much heat (in J) is required to increase the temperature of this kettle from 22.3°C to 99.5°C? _________________ J (c) How much heat (in J) is required to heat this kettle from 22.3°C to 99.5°C if it contains 1.10 L of water (density of 0.997 g/mL and a specific heat of 4.18 J/g·°C across the temperature range)? ______________________J