MISSED THIS? Watch IWE: Measuring AErxn in a Bomb Calorimeter, Read Section 7.5. You can click on the Review link to access the section in your e Text. Mothballs are composed primarily of the hydrocarbon naphthalene (C₁0 Hs). When 0.820 g of naphthalene burns in a bomb calorimeter, the temperature rises from 25.10 °C to 31.56 °C. Part A Find A Erxn for the combustion of naphthalene. The heat capacity of the calorimeter, determined in a separate experiment, is 5.11 kJ/°C. Express the change in energy in kilojoules per mole to three significant figures. View Available Hint(s) AErxn= Submit IVE ΑΣΦ ? kJ/mol

MISSED THIS? Watch IWE: Measuring AErxn in a Bomb Calorimeter, Read Section 7.5. You can click on the Review link to access the section in your e Text. Mothballs are composed primarily of the hydrocarbon naphthalene (C₁0 Hs). When 0.820 g of naphthalene burns in a bomb calorimeter, the temperature rises from 25.10 °C to 31.56 °C. Part A Find A Erxn for the combustion of naphthalene. The heat capacity of the calorimeter, determined in a separate experiment, is 5.11 kJ/°C. Express the change in energy in kilojoules per mole to three significant figures. View Available Hint(s) AErxn= Submit IVE ΑΣΦ ? kJ/mol

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

A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What quantity in moles of the unknown salt were used in the reaction?
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 ?
Magnesium metal is added to a coffee cup calorimeter containing 105.0 mL of 2.50 M hydrochloric acid. The temperature increased by 8.2°C. What lesson metal is placed in the calorimeter meter? Look at pic. The heat capacity and density a solution in the calorimeter is the same as those of water: 4.184 J/(g x degrees Celsius ) and 1.00 g/mL. Illinois it change in massive solution caused by adding magnesium and by escape of the hydrogen
When burning 0.25 g of CH3OH in a calorimeter bomb with a heat capacity of 1.50 kJ / 0C, it increases the temperature of the calorimeter bomb by 0.45 0C. How many kg of CH3OH (methyl alcohol) should be burned to obtain 2.76x105 kJ of heat? (CH3OH = 32 g / mol)
Question 11 X Incorrect. Isooctane, C3H18, is the basis of the octane rating system for gasoline because it burns smoothly, with minimal engine knocking. Pure isooctane is assigned a value of 100. Octane ratings are assigned to gasoline mixtures based on their ability to prevent knocking relative to isooctane. Estimate the energy released during the combustion of 1.00 mol of pure isooctane. Please note the combustion is exothermic process and the released energy is positive for the surroundings. -285.8 kJ
MISSED THIS? Watch KCV: Determining the Enthalpy of Reaction from Standard Enthalpies of Formation, IWE: AH*rxn and the Standard Enthalpies of Formation: Read Section 7.9. You can click on the Review link to access the section in your e Text. Propane (C₂Hg) burns according to the following balanced equation: C₂H3(g) +50₂(g) →3CO₂(g) + 4H₂O(g) Part A Calculate AHin for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/mol.) Express the enthalpy in kilojoules four significant figures. ▸ View Available Hint(s) AH VE ΑΣΦ ? kJ
Given the following equation: 2H3PO4 + 3Mg(OH)2 → 6 H2O + Ca3(PO4)2 + 450.8 kJ If 300 mL of 0.75 mols/L phosphoric acid solution, H3PO4, is mixed with 25.0 g of magnesium hydroxide, Mg(OH)2, predict the amount of energy released Note: the sign (-/+) is not relevant to the question. Your answer should follow the format: a) mols of H3PO4 b) maximum energy released if all of the H3PO4 reacts (with units) c) mols of Mg(OH)2 d) maximum energy released if all of the Mg(OH)2 reacts (with units) e) based on your answer to (b) and (d), how much energy will be released by this reaction based on the quantities of reactants indicated.
A sample of cold water was mixed with a sample of hot water inside a calorimeter, and the final temperature of the cold water was 40 °C. Which statement is true about the hot water in the calorimeter? It absorbed 40 joules. It absorbed 80 joules. Its final temperature was 80 °C. or Its final temperature was 40 °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
The citizens of the world burn the fossil fuel equivalent of 7 * 1012 kg of petroleum per year. Assume that all of this petroleum is in the form of octane (C8H18) and calculate how much CO2 (in kg) the world produces from fossil fuel combustion per year. (Hint: Begin by writing a balanced equation for the combustion of octane.) If the atmosphere currently contains approximately3 * 1015 kg of CO2, how long will it take for the world’s fossil fuel combustion to double the amount of atmospheric carbon dioxide?
Consider the following chemical reaction which produces nitric oxide from its constituent elements: N2 (g) + O2(g) → 2 NO (g) AH = 182.6 kJ/mol If nitrogen and oxygen were mixed and allowed to react under constant pressure conditions, which of the following statements must be true? Select as many answers as applicable however points will be deducted for incorrect guesses. ΔΗ = q This is an endothermic reaction The temperature of the surroundings would decrease The temperature of the surroundings would increase AH = AU
Silane, SiH4, burns according to the reaction, SiH4 + 2O2 → SiO2 + 2H2O, with ΔH° = –1429 kJ. How much energy in kJ is released if 18.01 g of silane is burned? Atomic Mass: Si: 28.086 g/mol H: 1.008 g/mol O: 15.999 g/mol Round your answer to 2 decimal places. Silane, SiH4, burns according to the reaction, SiH4 + 2O2 → SiO2 + 2H2O, with ΔH° = –1429 kJ. How much energy in kJ is released if 18.01 g of silane is burned? Atomic Mass: Si: 28.086 g/mol H: 1.008 g/mol O: 15.999 g/mol Round your answer to 2 decimal places.