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
When ammonia is oxidized it produces nitrogen monoxide and heat: 4NH3(g)+ 5O2(g)--> 4NO(g) +6H2O(g) "Triangle symbol"H degrees= -906kJ (a) Is the reaction endothermic or exothermic? Explain your answer. (b) If the reaction is carried out in a bomb calorimeter, will the temperature of the calorimeter increase or decrease? Explain your answer. (c) Is the internal energy of the products or reactants higher? Explain your answer.
Select the statement that is not supported by the following equation: q=0=(mwater)(cwater)( ΔTwater)+(mmetal)(cmetal)( ΔTmetal) The total change in heat is the sum of the changes in heat of water and a metal Energy is conserved. Energy is transferred between water and a metal. Energy is lost during a calorimetry experiment.
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
A 75g sample of a metal at temperature of 100℃ is placed in a calorimeter. The calorimeter contains 100g of water at a temperature of 34.4℃. The final temperature of the metal and the water in the calorimeter is 44.9℃. What is the specific heat of the metal? (cwater = 4.184J/g℃)
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
An 80 g sample of gas is heated from 25 C to 225 C. During this process, 346 J of work was done by the system and its internal energy is 8475 J. What is the specific heat capacity of the gas? (ans: 0.55 J/gC)
h5.) Most baths take 30.00 gallons of water. If the density of water is 1.000 g/mL, and 1gallon = 3.785 Liters, calculate how many grams of nitroglycerin (C3H5N3O9) it wouldtake to heat a bathtub of water from 25.00 °C to 75.00 °C. (Specific heat of water is still4.184 J/g°C).4 C3H5N3O9 12 CO2 + 10 H2O + 6 N2 + O2 H = -5678 kJ6.) If you used the nitroglycerin in problem 5 to fill a volume with the product gases, andthe total pressure is measured to be 5.31 atm, what is the partial pressure of each gas?(Explain what you can).