Calculate the heat capacity (j/C) of calorimeter Part A. Heat Capacity of CalorimeterHOTYour DataPartner's DataVolume (mL) of cold water50soVolume (mL) of hot waternst50ら0Density of waterP 1.00Mass (g) of cold water5050Mass (g) of hot watersosoInitial Temperature of cold water &Calorimeter20.8°し20.4°CInitial Temperature of Hot water59.60€55,3°CFinal Temperature after mixing34.6°-23.37.1F-IChange in Temperature for the hot waterChange in Temperature for the cold water &calorimeterー17.017.316.44Specific Heat capacity of water4.184 J/g * °C今。Heat Capacity (J/°C) of Calorimeteroolo2 sd lo vAve. Heat Capacity (J/°C) of CalorimeterCm x m m *Atm(If-In)

Answered: Image /qna-images/answer/7108b20b-4234-4a97-9b22-164e5ac2ed53.jpg

Part A. Heat Capacity of Calorimeter Your Data Partner's Data Volume (mL) of cold water 50 Volume (mL) of hot water 50 ら0 Density of water 1.00 Mass (g) of cold water 50 50 Mass (g) of hot water so so Initial Temperature of cold water & Calorimeter 20.2°C 20.4°C Initial Temperature of Hot water 59.60€ 55,3°C Final Temperature after mixing 34.6° 37.1 F-I Change in Temperature for the hot water -23.1 1し、4 ー17:6 17.3 Change in Temperature for the cold water & calorimeter Specific Heat capacity of water 4.184 J/g * °C P5. 2 Heat Capacity (J/°C) of Calorimeter Ave. Heat Capacity (J/°C) of Calorimeter Cm x M m *Atm -Cwy (If- In) = lom

Part A. Heat Capacity of Calorimeter Your Data Partner's Data Volume (mL) of cold water 50 Volume (mL) of hot water 50 ら0 Density of water 1.00 Mass (g) of cold water 50 50 Mass (g) of hot water so so Initial Temperature of cold water & Calorimeter 20.2°C 20.4°C Initial Temperature of Hot water 59.60€ 55,3°C Final Temperature after mixing 34.6° 37.1 F-I Change in Temperature for the hot water -23.1 1し、4 ー17:6 17.3 Change in Temperature for the cold water & calorimeter Specific Heat capacity of water 4.184 J/g * °C P5. 2 Heat Capacity (J/°C) of Calorimeter Ave. Heat Capacity (J/°C) of Calorimeter Cm x M m *Atm -Cwy (If- In) = lom

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.32E: Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special...

See similar textbooks

Similar questions

The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
Liquid hydrogen fluoride, liquid water,and liquid ammonia all have relatively high specific heats for suchsmall molecules. Speculate asto whythis might be so.
Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
Calculate the specific heat of a material if 288J of energy were required to heat 50.5g of the material from 298K to 330K. What are the units?
On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
What is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of 1550 torr, whileat the same time being cooled by removing 124.0J ofheat energy?
In a calorimetry 0.100 moles of NH4NO3(s) disolved in water. when the temperature decreeses 5.8 degrees celsius, and mass = 108g what is the molar entalphy change of solution? Specific heat capacity is same as water = 4.184 Jg-1K-1. Answer the question with errorslimits when the uncerainty of the temperature is 0.1 degrees celsius.
To determine the calorimeter constant of a coffee-cup calorimeter, 28 g of cold water was placed in the calorimeter. The initial temperature of the cold water and the calorimeter is 19.5ºC. A 28 g of hot water (initially at 62.2ºC) was placed in the calorimeter with cold water. Determine the experimental calorimeter constant, Ccal, if the final temperature after mixing is 37ºC. Use Cp of water = 4.184 J/gºC. Express your answer in 2 decimal places. Round your answer to 2 decimal places.
50.0 mL of 1.00 M HCl(aq) and 100.0 mL of 1.00 M NaOH(aq), both at 25.0oC, are added together in a calorimeter, the temperature of the mixture reaches a maximum of 29.6 oC. Determine the ΔH°rxn in kJ/mol. Assume no heat is lost to the calorimeter or the surroundings, and that the density and the heat capacity of the resulting solution are the same as water.