How much heat (in kJ) is released when 170 grams of CH4 is burned with 2000.grams of O2? If the answer is exothermic be sure your answer has the correct sign!CH4 + 202 --> CO + 2H20 AH = -803 kJ/molORC H4 + 2 02 right arrow CO + 2H2 O Delta H = -803 kJ/molHint: Determine the limiting reagent.Do not type units with your answer.Type your answer to three significant figures.If this question is on an exam on your scrap paper report your answer to the propernumber of significant figures but still type three significant figures online.Your Answer:

Answered: Image /qna-images/answer/5d2975aa-e6ac-4a40-a0cf-d759cfc75715.jpg

Answered: hic be sure your answer nas the correct…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 88QAP: A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is...

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Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C8H18() + 25 O2(g) 16 CO2(g) + 18 H2O() rH = 10,922 kJ/mol-rxn What is the enthalpy change if you burn 1.00 L of isooctane (d = 0.69 g/mL)?
A 70.0-g piece of metal at 80.0 °C is placed in loo g of water at 22.0 °C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6 °C. How much heat did the metal give up to the water? What is the specific heat of the metal?
Ethyl alcohol, C2H5OH, is the intoxicating agent in liquor. Burning 1.00 g of ethyl alcohol in an excess of oxygen at 23.28C and constant volume releases 29.52 kJ of heat. When 7.40 g of ethyl alcohol is burned in oxygen under the same conditions in a bomb calorimeter, the temperature of the bomb and water rises from 23.28C to 48.04C. The bomb holds 0.750 kg of water. (a) What is q for the combustion of the ethyl alcohol in the bomb calorimeter? (b) What is qH2O? (c) What is qcal? (d) What is the heat capacity of the calorimeter?
A compound is 82.7% carbon and 17.3% hydrogen, and has a molar mass of approximately 60 g/mol. When 1.000 g of this compound burns in excess oxygen, the enthalpy change is 49.53 kJ. (a) What is the empirical formula of this compound? (b) What is the molecular formula of this compound? (c) What is the standard enthalpy of formation of this compound? (d) Two compounds that have this molecular formula appear in Appendix G. Which one was used in this exercise?
Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride react, 1196 kJ of heat are evolved. (a) Write a thermochemical equation for the reaction. (b) What is Hf for ClF3?
Suppose you burned 1.500 g of benzoic acid, C6H5CO2H, in a constant-volume calorimeter and found that the temperature increased from 22.50 C to 31.69 C. The calorimeter contained 775 g of water, and the bomb had a heat capacity of 893 J/K. Calculate U per mole of benzoic acid.
You should use care when dissolving H2SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.2 g of concentrated H2SO4() was added (with stirring) to 135 g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 20.2 C to 28.8 C. Calculate the enthalpy change for the process H2SO4() H2SO4(aq), in kf/mol.
Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
A piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from 23.2 °C to 89.6 °C. (a) What is the specific heat of the substance? (b) If it is one of the substances found in Table 5.1, what is its likely identity?
A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is burned in a bomb calorimeter, sodium chloride does not burn. What is the percentage of sucrose in the sample if a temperature increase of 1.67C is observed when 3.000 g of the sample are burned in the calorimeter? Sucrose gives off 5.64103kJ/mol when burned. The heat capacity of the calorimeter and water is 22.51 kJ/C.

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