A 0.2415g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 The temperature increases by1.978 °C.Part 1 of 2kJCalculate the heat associated with the burning of Mg inBe sure your answer has the correct number of significant digits.gPart 2 of 2kJg☐ x10☑Calculate the heat associated with the burning of Mg inkJmolBe sure your answer has the correct number of significant digits.KJmolx10☑

for given magnesium sample Heat on changing given temperature difference is,1. Heat = 1.44 KJ/g2.…

Answered: A 0.2415 g sample of solid magnesium 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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 64E: A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed...

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Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU. (a) How many joules are in one therm? (1J=9.48104BTU) (b) When propane gas, C3H8, is burned in oxygen, CO2 and steam are produced. How many therms of energy are given off by 1.00 mol of propane gas?
Acetic acid, HC2H3O2, is responsible for the sour taste of vinegar. Combustion of acetic acid gives off 14.52 kJ/g of heat. When 15.00 g of acetic acid is burned in a bomb calorimeter (heatcapacity=2.166kJ/C) containing 0.800 kg of water, the final temperature in the calorimeter is 64.14C. What was the initial temperature of the calorimeter?
Swimming Pool A swimming pool measuring 20.0m12.5m is filled with water to a depth of 3.75m. If the initial temperature is 18.4°C, how much heatmust be added to the water to raise its temperature to29.0°C? Assume that the density of water is 1.000 g/mL.
9.74 Without looking up any numerical data or doing calculations, predict whether the following enthalpy changes should he positive, negative, or zero. (a) Hf for H2(g) (b) Hf for O(g) (c) Hfusion for H2O (d) Hcombusion for C3H8(g)
An aluminum kettle weighs 1.05 kg. (a) What is the heat capacity of the kettle? (b) How much heat is required to increase the temperature of this kettle from 23.0 C to 99.0 C? (c) How much heat is required to heat this kettle from 23.0 C to 99.0 C if it contains 1.25 L of water (density of 0.997 g/mL and a specific heat of 4.184 J/g C)?
9.90 Many engineering designs must incorporate ways to dissipate energy in the form of heat. Water evaporators are common for this task. (a) What property of water makes it a good material for evaporators? {b} If an application could not use water, hut instead was forced to use a material with a value for the property in part (a) that was one half that of water, what changes would need to be made in the design?
A piece of iron was heated to 95.4C and dropped into a constant-pressure calorimeter containing 284 g of water at 32.2C. The final temperature of the water and iron was 51.9C. Assuming that the calorimeter itself absorbs a negligible amount of heat, what was the mass (in grams) of the piece of iron? The specific heat of iron is 0.449 J/(gC), and the specific heat of water is 4.18 J/(gC).
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An iron skillet weighing 1.63 kg is heated on a stove to 178C. Suppose the skillet is cooled to room temperature, 21C. How much heat energy (in joules) must be removed to affect this cooling? The specific heat of iron is 0.449 J/(gC).
The complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene consumed. How many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal water by 10.0c if the process is 80.0% efficient? Assume the density of water is 1.00 g/cm3
A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed in a container of water at 22.3C. The final temperature of the water and copper is 24.9C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?
Colorless nitric oxide, NO, combines with oxygen to form nitrogen dioxide, NO2, a brown gas. 2NO(g)+O2(g)2NO2(g);H=114kJ What is the enthalpy change per gram of nitric oxide?

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