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
In a calorimeter, a 75.0 g piece of metal at 98.6 *C is submerged in 100.0 g of water, that is initially at 21.8 *C. When the metal and water reach thermal equilibrium, the temperature is 26.2 *C. What was the heat capacity of the metal (3 sig figs)?
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
A piece of iron (specific heat, 0.444 J/g•°C) is added to 127.31 grams of water (specific heat, 4.184 J/g•°C) in a calorimeter. The water was initially at a temperature of 27.6°C and the iron was initially at 143.9°C. If the final temperature of the system is 33.8°C, what is the mass of the iron? Report your answer with 3 significant figures.
Please assist me with my practice question. The combustion of butane is shown by the following equation: 2C4H10 (l) + 13O2 (g) → 8CO2 (g) + 10H2O(g) Use the following data and the summing method to find the heat of reaction for the above equation. Note: Show all calculations, follow the rules of significant figures, and box your final answer. C(s) + O2 (g) → CO2 (g) + 393 kJ H2 (g) + ½O2 (g) → H2O(g) + 242 kJ 4C(s) + 5H2 (g) → C4H10 (g) + 125 kJ
4) Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat? Explain your answer based on the specific heat capacity value. Specific Heat (J/g°C) 0.903 J/g°C 0.385 J/g°C 0.79 J/g°C 0.128 J/g°C 0.235 J/g°C Substance Amount in Grams Al 50.0 g 50.0 g 25.0 g 25.0 g 25.0 g Cu Granite Au Ag
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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
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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