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. Top fuel dragsters and funny cars burn nitromethane as fuel according to the following balanced combustion equation: 2CH₂NO₂ (1) + O₂(g) → 2CO₂(g) + 3H₂O(l) + N₂(g), AH = -1418 kJ The standard enthalpy of combustion for nitromethane is -709.2 kJ/mol. The standard enthalpies of formation are -393.5 kJ/mol for CO₂(g) and -285.8 kJ/mol for H₂O(1) Part A Calculate the standard enthalpy of formation (AHr) for nitromethane. Express your answer in kilojoules per mole to one decimal place. ΑΣΦ AH₂ = ? kJ/mol

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. Top fuel dragsters and funny cars burn nitromethane as fuel according to the following balanced combustion equation: 2CH₂NO₂ (1) + O₂(g) → 2CO₂(g) + 3H₂O(l) + N₂(g), AH = -1418 kJ The standard enthalpy of combustion for nitromethane is -709.2 kJ/mol. The standard enthalpies of formation are -393.5 kJ/mol for CO₂(g) and -285.8 kJ/mol for H₂O(1) Part A Calculate the standard enthalpy of formation (AHr) for nitromethane. Express your answer in kilojoules per mole to one decimal place. ΑΣΦ AH₂ = ? 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...

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Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining
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
n the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 63.03 grams of chromium to 98.03 °C and then drops it into a cup containing 79.71 grams of water at 23.19 °C. She measures the final temperature to be 28.85 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of chromium. Specific Heat (Cr) = ____________J/g °C.
The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5 × 104 kJ of heat? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ
Propane (C3H8) is the commonly used fuel in our barbeques at home. It is a great fuel because it will release 2220 kJ of energy for every mole that combusts. A. Write the balanced reaction for the combustion of propane. B. When 50.0g of propane cobusts, how much energy is released? C. Is this reaction exothermic or endothermic? Provide evidence.
CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol Using the equation above, how many grams of water will form if 655 kJ of energy was released.
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
Please help with question 2!