The heat capacity of a bomb calorimeter was determined by burning 6.79 g methane (energy of combustion CH4) in the bomb. The temperature changed by 10.8°C. -802 kJ/mol a. What is the heat capacity of the bomb? b. A 12.6-g sample of acetylene, C,H2, produced a tempera- ture increase of 16.9°C in the same calorimeter. What is the energy of combustion of acetylene (in kJ/mol)? the tem-

The heat capacity of a bomb calorimeter was determined by burning 6.79 g methane (energy of combustion CH4) in the bomb. The temperature changed by 10.8°C. -802 kJ/mol a. What is the heat capacity of the bomb? b. A 12.6-g sample of acetylene, C,H2, produced a tempera- ture increase of 16.9°C in the same calorimeter. What is the energy of combustion of acetylene (in kJ/mol)? the tem-

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...

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A serving of Chocobits cereal is 122 g.A 1.00-g sample of the cereal is burned in a bomb calorimeter that has a heat capacity, C, of 8.50 kJ K-1, causing the temperature to increase from 25.0°C to 25.8°C. Calculate the energy of Chocobits in Calories per serving to three significant figures. 1 Cal = 4.184 kJ
An important flavor component of vanilla extract is vanillin (C8H8O3, molar mass = 152.15 g/mol). When vanillin burns in a bomb calorimeter with a heat capacity of 14.18 kJ/°C, the temperature increases from 25.22°C to 31.57°C. If the heat of combustion of vanillin is -3,760 kJ/mol, what mass of vanillin (in g) was combusted? Please give your answer to 2 decimal places.
4.51 g of octane, C8H18, reacts with excess oxygen in a bomb calorimeter. The heat capacity of the calorimeter is 6.97 kJ/°C and the temperature increases by 72.0°C. How much heat, in units of kJ/mol, was absorbed by the bomb calorimeter?
The combustion of 0.1559 g benzoic acid increases the temperature of a bomb calorimeter by 2.52°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2138-g sample of vanillin (C3H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.22°C. What is the energy of combustion per gram of vanillin? Energy kJ/g %3D Per mole of vanillin? Energy = kJ/mol
2. A sample of nickel is heated to 99.8°C and placed in a coffee cup calorimeter containing 150.0 g water at 23.5°C. After the metal cools, the final temperature of metal and water mixture is 25.0°C. If the specific heat capacity of nickel is 0.444 J/°C a. what mass of nickel was originally heated? Assume no heat loss to the surroundings.
A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś
pt pt pt pt pt pt pt pt pt pt pt pt pt pt You should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.8 g of concentrated H₂SO4() was added (with stirring) to 140. g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 21.0 °C to 30.3 °C. Calculate the enthalpy change for the process H₂SO4(l) → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change = kJ/mol ?
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
metal X =51.0g; specific heat capacity =0.44 J/C If metal X is heated to 86C and put into a calorimeter containing water (she=4.18 J/g°C ) at 23C. The final temperature of the water becomes 31C. What is the mass of water?
[11] A 10.00 g sample of a metal alloy was heated to 88.99 °C. It is then quickly dropped into 40.0 g of water in a calorimeter. The water temperature rises from 19.73 °C to 24.23 °C. Calculate the specific heat of the alloy. [Specific Heat of Water = 4.184 J/g °C and Heat Capacity of Calorimeter = 12.6 J/°C]
110. Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by qui- none in certain enzymes allows plants to take water, carbon dioxide, and the energy of sunlight to create glucose. A 0.1964-g sample of quinone (C,H,O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/°C. The tempera- ture of the calorimeter increases by 3.2°C. Calculate the en- ergy of combustion of quinone per gram and per mole. 111 A I TO
In a calorimeter, a 2.0 g sample of magnesium is burned to form MgO. In doing so, 25.5 kJ of energy are released. What is the Heat of Combustion in kJ/mol of magnesium? с 306.2 1.54 x 1025 0.0392 514 25.5