A 26.1 g peice of brass alloy with a specific heat capacity of 0.377 J g1 °c1, initially at 120.3 °C, is cooled by submurging it into 55.1 g of water (specific heat capacity=4.184 J g 1 °c-1) at 22.9 °C, in an insulated container. Part A What is the final temperature of both substances at thermal equilibrium? Express your answer using three significant figures. T = °C

A 26.1 g peice of brass alloy with a specific heat capacity of 0.377 J g1 °c1, initially at 120.3 °C, is cooled by submurging it into 55.1 g of water (specific heat capacity=4.184 J g 1 °c-1) at 22.9 °C, in an insulated container. Part A What is the final temperature of both substances at thermal equilibrium? Express your answer using three significant figures. T = °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

A chemist wastes a delicious brownie by burning it in a bomb calorimeter. Before burning, the brownie weighed 21.80 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.87 ∘C. The known heat capacity of the calorimeter that was used was 42.73 kJ/∘C. What is the energy content, in kJ/g, of this brownie? (Enter your answer with no units. Since we are describing the energy content of the brownie, please ENTER THIS NUMBER AS A POSITIVE NUMBER, not a negative number!)
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
the molar heat capacity of iron is 25.10 J mol –1 K–1 . A 25.0 g ball is heated until it is glowing red (to a temperature of 400.°C). It is dropped into a 50.0 mL container of water at 25.0°C. If the density of water is 0.997 g mL–1 , and the molar heat capacity of water is 4.186 J g–1 K–1 , what temperature (in K) will the ball and water equilibrate to? A) 338 B) 300 C) 317 D) 359 E) 342
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.88 kg sample of C,H0, from 35.8 °C to 51.4 °C. The experiment shows that 2.34 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H00,? Round your answer to 2 significant digits. |J-mol 1 - 1 •K х10
4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)
1. 40.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 20.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H,0(1), c = 4.18 J/gx°C; H,O(s) → H,O(1) AH= 6.02 kJ/mol)
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
Part A A silver block, initially at 55.8 °C, is submerged into 100.0 g of water at 24.1°C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.3 °C. The specific heat capacities for water and silver are = 4.18 J/(g ·°C) and 0.235 J/(g·°C). What is the mass of the silver block? Express your answer to two significant figures and include the appropriate units. Cs, water • View Available Hint(s) Cs, silver = HA ? Value Units m =