The symbol AH represents enthalpy change Select one: O True False In a closed system, at 25°C and 1 atmosphere of pressure, a small sample of methane is combusted. All of the methane is reacted according to the following equation: CH4(9)+ 20₂(g) → CO₂(g) + 2H₂O(1) In order to determine the enthalpy change of the system, must be assumed that the products are also at 25°C and 1 atmosphere of pressure. Select one: O True O False In Question 11, the kinetic energy of the products will be the same as the kinetic energy of the reactants. Select one: O True False

The symbol AH represents enthalpy change Select one: O True False In a closed system, at 25°C and 1 atmosphere of pressure, a small sample of methane is combusted. All of the methane is reacted according to the following equation: CH4(9)+ 20₂(g) → CO₂(g) + 2H₂O(1) In order to determine the enthalpy change of the system, must be assumed that the products are also at 25°C and 1 atmosphere of pressure. Select one: O True O False In Question 11, the kinetic energy of the products will be the same as the kinetic energy of the reactants. Select one: O True False

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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Butane, C4H10, is widely used as a fuel for disposable lighters When one mole of butane is burned in oxygen, carbon dioxide and steam are formed and 2654.3382 kJ of heat are evolved.. C4H10 (9) + O₂(g) → 4CO₂(g) +5H₂O(1) The standard enthalpies of formation of CO₂ and H₂O are: CO2(g)=-394.87 kJ/mol H₂O(1)=-285.59 kJ/mol Calculate the standard heat of formation of butane. (Round answer to the second decimal place)
2.000 g of Compound X with molecular formula C5H₁0 are burned in a constant-pressure calorimeter containing 45.00 kg of water at 25 °C. The temperature 10 of the water is observed to rise by 0.4696 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits. 0 00 X Ś x10
In this experiment you will place a sample of your salt in water in a constant pressure calorimeter. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the number of moles of SrCl2? 4.368 g SrCl2 x ( 1 mol SrCl2 / 123.073 g SrCl2 ) = 0.035491131 mol SrCl2 a. 0.035491 mol SrCl2 b. none of these c. 0.035 mol SrCl2 d. 0.03 mol SrCl2 e. 0.0355 mol SrCl2 f. 0.04 mol SrCl2 g. 0.035491131 mol SrCl2 h. 0.03549 mol SrCl2
Let's use our knowledge of constant volume (bomb) calorimetry to determine the heat energy in a given food sample, say a hamburger. A typical hamburger has a serving size of 105 g and consists of approximately 20% protein (21.0 g), 33% fat (34.7 g), and 47% carbohydrate (49.3 g). Assume that the heat capacity of the bomb calorimeter is 8.39 kJ K-¹, and the increase in water temperature was 13.2 K. Q5.38 Homework Unanswered How many Calories (Cal) are in the hamburger described above? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered • 4 attempts left Submit
Find the molar enthalpy of combustion in kJ/mol of glucose at some temperature and pressure C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) given that in an experiment under the same conditions the combustion of 0.108 g of glucose raised the temperature of a calorimeter with total heat capacity C= 1.155 kJ/°C by 1.31 °C. The molar mass of glucose is 180.1 g/mol. Ignore the heat absorbed by the combustion products; assume this is negligible, and all heat went into the calorimeter itself. Give the answer with 5 or more significant figures.
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12.00 g of Compound with molecular formula C4h8 are burned in a constant-pressure calorimeter containing 15.00 kg of water at 25 °C. The temperature of the water is observed to rise by 8.603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. calorimeter itself.)
Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H,O(g) –→ CO,(g) + H,(g) AHân = kJ
Determine the enthalpy for the production of 5.0 g of H2 in the following target equation, making use of the known equations given below. CH4 (g) + NH3 (g) → HCN(g) + 3H2 (g) Using the following given equations: N2 (g)+3H2 (g) → 2NH3 (g) ΔH=− 91.8kJ C(s)+2H2 (g) → CH4 (g) ΔH=− 74.9kJ H2(g) + 2C(s) + N2 (g) → 2HCN(g) ΔH= + 270.3 kJ
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.1250 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.200×103 g of water. During the combustion the temperature increases from 23.58 to 26.40 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 979.8 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.C6H12O6(s) + 6O2(g) 6 H2O(l) + 6 CO2(g) + Energy
5.000 g of Compound X with molecular formula C,H, are burned in a constant-pressure calorimeter containing 20.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.556 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. ? olo :