Phereseadula has to determine the specific heat capacity of milk. He uses a constant volume calorimeter with a heat capacity of 758 J/K and the combustion of acetylene (C2H2) to do the experiment: 2C2H2(g) + 502(g) 4CO2(g) + 2H20(g) ---- ArH = -2610kJ The calorimeter is filled with 1.190L of milk (instead of water). The density of milk is 1.034 g/ cm3. When 4.413 g of acetylene is burned in excess oxygen in the reaction vessel (bomb) of the calorimeter, the temperature of the milk and the bomb increased from 22.5°C to 61.9°C. The heat absorbed by the bomb is:

Phereseadula has to determine the specific heat capacity of milk. He uses a constant volume calorimeter with a heat capacity of 758 J/K and the combustion of acetylene (C2H2) to do the experiment: 2C2H2(g) + 502(g) 4CO2(g) + 2H20(g) ---- ArH = -2610kJ The calorimeter is filled with 1.190L of milk (instead of water). The density of milk is 1.034 g/ cm3. When 4.413 g of acetylene is burned in excess oxygen in the reaction vessel (bomb) of the calorimeter, the temperature of the milk and the bomb increased from 22.5°C to 61.9°C. The heat absorbed by the bomb is:

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

The following thermochemical equation is for the reaction of Fe3O4(s) with hydrogen (g) to form iron(s) and water(g). Fe3O4(s) + 4H₂(g) 3Fe(s) + 4H₂O(g) ΔΗ = 151 kJ When 81.5 grams of Fe3O4(s) react with excess hydrogen (g), kJ of energy are 0. 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.
C50H 102 is burned in a bomb calorimeter that has a heat capacity of 45.71/ When the temperature increases from 19.20 °C to 40.55 °C, the change in internal energy is determined to be -573.9 K. What is the mass of C50H102 which was burned in the combustion reaction? mol
Find the mass of water that vaporizes when 2.10 kg of mercury at 205 °C is added to 0.10 kg of water at 30°C. Assume the following: Cmercury (specific heat capacity of mercury) - 139 J/(kg.°C): Cwater (specific heat capacity of water) = 4186 J/(kg.°C); and L, (water) = 2.26x106 J/kg
ap lut CX ter tion A101.6gram sample of an unknown metal at83.0°C was mixed with318.0grams of20.1°C water in a coffee-cup calorimeter. The temperature of the mixture equilibrated at32.8°C. What is the specific heat of this metal in calories/(g°C)? calories/(g°C) i eTextbook and Media
Give detailed Solution (don't give Handwritten answer ,don't use Ai for answering this
The following thermochemical equation is for the reaction of Fe,0, (s) with hydrogen (g) to form iron(s) and water (g). Fe₂O₂ (s) + 4H₂(g) 3Fe(s) + 4H₂O(g) AH = 151 kJ Use the References to access important values if needed for this question. When 86.8 grams of Fe₂O4(s) react with excess hydrogen(g). 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. Submit Answer kJ of energy are
A food product containing 82% moisture content is being frozen. Predict the specific heat of the product at -8 ° C when 82% of the air is frozen. The specific heat of the dry product is 2.5 kJ / (kg ° C). It is assumed that the specific heat of water at -10 ° C is the same as that of water at 0 ° C, and that the specific heat of ice follows the function Cp ice = 0.0062 T frozen + 2.0649. Cp of frozen product = answer J / kg ° C.
How much heat evolves when 216 mL of benzene is consumed in the combustion reaction below. The density of benzene is 0.88g/mol. The molar mass of benzene is 78.11 g/mol. Delta H Reaction = -6278 kJ2C6H6(l)+15O2(g)—>12CO2(g)+6H2O(g)
How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar? The reaction we performed was: Na(s) + H2O(l) NaOH(aq) + 1/2H2(g) qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is: 0 = qsystem = qreaction + qwater qreaction = -qwater qreaction = -mwater*Cwater*Twater The data from the demonstration was: (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g How many moles of sodium were added to the water (in moles)?
In a coffee cup calorimeter, 10.0mL of 1.00M AgNo3 and 10.0mLof 1.00M NaCl are mixed and the following reaction occurs (assume reaction goes to completion) Ag+ (aq) + Cl-(aq) ----> AgCl(s) The 2 solutions are intitially at 25.0C and the final temperature is 36.2C. Assuming density of the solution is 1.00g/mL and the heat capactity of the solution is 4.18J/K/g. Calculate q for the reaction in KJ
How much energy is liberated when 600.2g of O2 is reacted with propane in a combustion tank. Assume: C3H8(g) + 5CO2(g)—> 3CO2(g) + 4H2O(g) ; delta H reaction= -2044 kJ