(b) Calculate the gross calorific value of a coal from the following data: Mass of coal = 0.5 g Water equivalent of calorimeter = 2000 g Specific heat of water = 4.187 kJ/kg/°C Rise in temperature of water = 5.4°C

(b) Calculate the gross calorific value of a coal from the following data: Mass of coal = 0.5 g Water equivalent of calorimeter = 2000 g Specific heat of water = 4.187 kJ/kg/°C Rise in temperature of water = 5.4°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

Volume of cool water (mL) Volume of hot water (mL) Initial temperature of cool water (°C) Initial temperature of hot water (°C) Final temperature of water in calorimeter (°C) Temperature change for cool water (°C) Temperature change for calorimeter (°C) Temperature change for hot water (°C) Heat change for cool water (J) Heat change for hot water Heat change for calorimeter (J) Heat capacity of calorimeter (J/°C) Trial 1 50.0 47.5 24.3 38.9 37.0 Trial 2 50.0 46.1 24.9 35.0 33.7 Trial 3 50.0 44.8 23.3 33.8 30.8
A gas expands and does work on the surroundings equal to 3.55 L atm. At the same time, it releases 540.4 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
A coffee cup calorimeter, including that water it contains, has a heat capacity of 425 J/K, and is initially at a temperature of 23.07 C. A 16.9 gram piece of nickel metal, initially at a temperature of 4.0°C is placed in the calorimeter. The final temperature of the calorimeter and the metal is 22.74°C. What is the specific heat of nickel metal (in Jg1 K-1)? 27 O0.44 1.4 O 25 O 145
I need the answer as soon as possible
When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ
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)
2. Slaked lime (Ca(OH)2(s)) is produced when lime (calcium oxide, Cao (s)) reacts with liquid water. 65.2 kJ of heat is released for each mol of Ca(OH)2 that is produced. (a) Write a thermochemical equation for the reaction. (b) What is the enthalpy change when 523.3 kg of lime reacts with excess water?
A 88.8 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 24.8°C. Ignoring significant figures, calculate the mass of water in the calorimeter.
3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.) J What is the specific heat (in J/g·°C) of the metal? J/g·°C 4. A 0.528 g sample of KCl is added to 51.7 g of water in a calorimeter. If the temperature decreases by 1.07°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? J Is the reaction exothermic or endothermic? exothermicendothermic 5. When 2.56 g of methane burns in oxygen, 128 kJ of heat is produced. What is the enthalpy of combustion (in kJ) per mole of methane under these conditions? kJ/mol methane 6. Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much…
2. A piece of Cu metal is heated in a test until the temperature reaches 96 °C and dropped into a calorimeter with 50.0 ml of water with a temperature of 27°C. after the addition of the metal, temperature of water in the calorimeter rises to 29 °C What is the mass of Cu added?
A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
Express the quantity in the unit indicated and designate whether this heat is gained or lost by the substance a. The quantity of heat in calories when 162.5 grams of water undergoes a temperature decrease from 45.84 C to 40.00 C. b. The quantity of heat in Kilojoules when 43.5 Kg of chloroform ,CHCl3 has its temperature changed from 16.8 C to 22.3 C ( sp ht of CHCl3 = 0.971 KJ/kg- C)