Part A Two substances, A and B, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of substance A is 6.29 g and its initial temperature is 20.7 °C . The mass of substance B is 25.9 g and its initial temperature is 52.5 °C. The final temperature of both substances at thermal equilibrium is 46.0 ° C. If the specific heat capacity of substance B is 1.17 J/(g.°C), what is the specific heat capacity of substance A? Express your answer in joules per gram per degree Celsius. • View Available Hint(s) V AE ? CsA = J/(g. °C)

Part A Two substances, A and B, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of substance A is 6.29 g and its initial temperature is 20.7 °C . The mass of substance B is 25.9 g and its initial temperature is 52.5 °C. The final temperature of both substances at thermal equilibrium is 46.0 ° C. If the specific heat capacity of substance B is 1.17 J/(g.°C), what is the specific heat capacity of substance A? Express your answer in joules per gram per degree Celsius. • View Available Hint(s) V AE ? CsA = J/(g. °C)

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

100.0 mL of cold water at 20.5 oC was poured into a styrofoam coffee cup calorimeter. After adding 100.0 mL of hot water at 30.5 oC and mixing it thoroughly, the temperature of the mixture was found to 24.7 oC. Find the heat capacity of the calorimeter. [Specific heat capacity of water is 4.184 J/goC. Assume density of water is 1.0 g/mL at both temperatures.]
please help with this question
A candy bar has a total mass of 75.0 grams. In a calorimetry experiment, a 1.25-g sample of this candy bar was burned in a calorimeter surrounded by 1000 g of water. The temperature of the water in contact with the burning candy bar was measured and found to increase from an initial temperature of 21.2°C to a final temperature of 24.3°C. a. Calculate the amount of heat in calories released when the 1.25-g sample burned. (show the work you did)
A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)?0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A piece of titanium metal with a mass of 21.6 g is heated in boiling water to 99.5 °C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.8 °C. When thermal equilibrium is reached, the final temperature is 24.5 °C. Calculate the specific heat capacity of titanium. (The specific heat capacity of liquid water is 4.184 J/g. K.) Specific heat capacity= J/g. K
12. When 30.0 mL of 1.00 M HCl(aq) and 45.0 mL of 1.00 M NaOH(aq), both at 21.0 °C, are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 24.0° What is the amount of heat produced by this reaction? The mixture has a specific heat of 4.184 J/g °C and density of 1g/mL. Show work and write your answers in 4 significant figures. Box in your final answer. HCl(aq) + NaOH(aq) --> NaCl(aq) + H₂O(1)
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 19.5 g.19.5 g. The temperature of the substance increases by 16.1 ∘C16.1⁢ ∘C when 73.8 J73.8 J of heat is added to the substance. What is the most likely identity of the substance?
A particular container holds 3.77 mol of neon gas. The volume of this container can be altered by sliding a piston in or out. The volume is changed from 8.60 L to 12.20 L while at the same time the temperature is changed from 303 K to 345 K. The molar heat capacity, Cym, for neon is 12.47 J/(mol · K). Assume that this value will not change over the given temperature range. What is the change in entropy for the gas? AS = J/K TOOLS x10 MacBook Pro
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 14.5 g.14.5 g. The temperature of the substance increases by 15.3 ∘C15.3 ∘C when 85.4 J85.4 J of heat is added to the substance.
We place a metal rod weighing 5.00 g with a specific heat capacity of 0.320 J/K/g in 20.4 mL of water. The specific heat capacity of water is 4.184 J/K/g and we make the approximation that its density is exactly 1.000 g/mL. The water has an initial temperature of 20.0 oC and the metal rod has an initial temperature of 88.0 oC. What is the final temperature (in oC) of the water and metal rod?
A nickel at 30 °C is dropped into a glass of 15.0 g soda at 3.0 °C, if the heat capacity of the nickel is 4.40 J/°C, the heat capacity for the glass is 11.1 J/°C, and the soda has the same specific heat capacity as water (4.184 J/g°C), what is the final temperature of the mixture?
a) Two substances, lead and granite, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of lead is 20.4 gg and its initial temperature is 55.7 ∘C∘C. The mass of granite is 18.7 gg and its initial temperature is 22.7 ∘C∘C. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of lead is 0.128 J/(g⋅∘C)J/(g⋅∘C); the specific heat capacity of granite is 0.79 J/(g⋅∘C)J/(g⋅∘C).) b) A 4.03 gg sample of gold, initially at 70.4 ∘C∘C, is submerged into 60.8 gg of water at 17.8 ∘C∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of gold is 0.128 J/(g⋅∘C)J/(g⋅∘C);the specific heat capacity of water is 4.18 J/(g⋅∘C)J/(g⋅∘C).)