A piece of unknown substance weighs 44.7 g andrequires 2110J to increase its temperature from 23.2°C to 89.6 °C. If it is one of the substances found infollowing table, what is its likely identity?Specific Heats of Common Substances at 25 °C and 1 barSubstanceSymbol (state)Specific Heat (Jig °C)Не(9)H2O()helium5.193water4.184ethanol2.376H2O(s)H2O(g)N2(g)ice2.093 (at -10 °C)water vapor1.864nitrogen1.040air1.007oxygenO9)0.918aluminumAl(s)CO2(9)Ar(g)Fe(s)0.897carbon dioxide0.853argon0.522iron0.449соррerCu(s)0.3850.130Pb(s)Au(s)leadgold0.129siliconSi(s)0.712Ar(g)Si(s)O Al(s)

Heat absorbed = m Cp ∆T Cp is specific heat capacity. m is mass of substance.

A piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from 23.2 °C to 89.6 °C. If it is one of the substances found in following table, what is its likely identity? Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol (state) Specific Heat (Jig °C) Не (9) H20() helium 5.193 water 4.184 2.376 2.093 (at -10 °C) ethanol ice H20(s) water vapor 1.864 (6)0H 1.040 nitrogen N2(g) air 1.007 O9) Al(s) CO2(9) охудen 0.918 aluminum 0.897 carbon dioxide 0.853 Ar(g) Fe(s) Cu(s) argon 0.522 iron 0.449 copper 0.385 lead Pb(s) 0.130 gold Au(s) 0.129 silicon Si(s) 0.712 O Ar(g) Si(s)

A piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from 23.2 °C to 89.6 °C. If it is one of the substances found in following table, what is its likely identity? Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol (state) Specific Heat (Jig °C) Не (9) H20() helium 5.193 water 4.184 2.376 2.093 (at -10 °C) ethanol ice H20(s) water vapor 1.864 (6)0H 1.040 nitrogen N2(g) air 1.007 O9) Al(s) CO2(9) охудen 0.918 aluminum 0.897 carbon dioxide 0.853 Ar(g) Fe(s) Cu(s) argon 0.522 iron 0.449 copper 0.385 lead Pb(s) 0.130 gold Au(s) 0.129 silicon Si(s) 0.712 O Ar(g) Si(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

Find the heat of metal and the specific heat capacity (below are the values) Mass of metal 23.2038g volume of water 100.0 mL Initial temperature of water 25.01 degrees Celcius Initial temperature of Metal 200.00 degrees celcius Max final temperature of water and metal 28.75 degrees celcius mass of water 99.71g change in temperature for water 3.74 degrees celcius Heat of water 156 Joules Change in temperature for metal -171.25 Degrees celcius
22.009 g of a metal at 100.15°C was added to 15.6 g of water at 18.01°C. The temperature of the mixture rose to 28.36°C. What is the specific heat of the metal? SH20 = 4.184 J/g°C Your Answer: Answer units
A piece of unknown metal with a mass of 23.78 g is heated in boiling water to 97.4°C and then dropped into a coffee cup calorimeter containing 72.71 g of water at 13.65°C. When thermal equilibrium is reached, the final temperature is 24.79°C. Calculate the specific heat capacity of the unknown metal. The specific heat of water is 4.184 J/g/°C. Round your answer to 2 decimal places.
A 0.2415 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 The temperature increases by 1.978 °C. Part 1 of 2 kJ Calculate the heat associated with the burning of Mg in Be sure your answer has the correct number of significant digits. g Part 2 of 2 kJ g ☐ x10 ☑ Calculate the heat associated with the burning of Mg in kJ mol Be sure your answer has the correct number of significant digits. KJ mol x10 ☑
A calorimetry experiment was done on a mystery piece of metal and the data was recorded in the table below. Measurement 89.20 g Mass of the metal Initial temperature of the metal Mass of the water Initial temperature of the water Final temperature of the water 98.1 °C 47.50 g 22.5 °C 28.2 °C What was the specific heat of the mystery metal? (CH20 = 4.181 J/gºC ) Round your answer to 2 decimal places.
A piece of metal weighing 146.7 g was heated from 32.0 °C to 56.2 °C. If the amount of heat needed was 1363.3 J, calculate the specific heat of the metal. What is the identity of the metal? 20 Specific Heats of Selected Metals Smetal, J/g-°C Metal 0.901 Smetal, J/g-°C 0.449 Metal Al Fe Cu 0.384 Ni 0.444 Si 0.711 Sn 0.226 Zn 0.389 Mn 1.02
The combustion of butane produces heat according to the equation2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(l) ΔH = -5,314.0 kJ What is the change in heat if 13.98 g C4H10 (58.12g/mol) reacts?(Answer should have one place after the decimal. Watch the sign)
Use the References to access important values if needed for this question. The following thermochemical equation is for the reaction of methane(g) with water(g) to form hydrogen(g) and carbon monoxide(g). CH4(g) + H20(g)3H2(g) + CO(g) →3H2(g) + CO(g) AH = 206 kJ When 6.16 grams of methane(g) react with excess water(g), kJ of energy are Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.
5(a)
A series of equal-mass samples of the five materials listed in the table are brought from room temperature to 100. °C. Which sample required the least amount of energy (J) to reach the final temperature? Material Specific heat (J/g•°C) Al (aluminum) 0.903 Pyrex glass 0.75 Fe (iron) 0.449 Pb (lead) 0.128 water; H2O (l) 4.18
A chemist carefully measures the amount of heat needed to raise the temperature of a 284.0 mg sample of a pure substance from 51.6 °C to 61.2 °C. The experiment shows that 13. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. - 1
How much heat is given off to the surroundings when 6 g of aluminum reacts according to the following equation? Express your answer correctly rounded to two decimal places.2 Al + Fe2O3 Al2O3 + 2 Fe ΔH°rxn = -849 kJ. kJIf all of the heat generated by the reaction was absorbed by one liter of room temperature water, what would be the highest temperature the water could reach? Express your answer correctly rounded to two decimal places. °CWhile writing this question, I had to take into account that the final temperature reachable in the previous question could not exceed the boiling point of water. Given this information, what is the highest whole number amount of aluminum that could have been used for this question? Enter only a number for your answer. g