### Understanding Enthalpy of Reaction from Standard Enthalpies of Formation#### Background InformationHydrazine (N₂H₄) is a fuel used by some spacecraft. It is commonly oxidized by N₂O₄ according to the reaction:\[ \text{N}_2\text{H}_4(l) + \text{N}_2\text{O}_4(l) \rightarrow 2\text{N}_2(g) + 2\text{H}_2\text{O}(g) \]#### Table of Standard Enthalpies of FormationThe following table provides the standard enthalpies of formation (\( \Delta H_f^\circ \)) for various substances:| Substance | \( \Delta H_f^\circ \) (kJ/mol) ||-----------|---------------------------------|| N₂(g) | 0.0 || NH₃(g) | -45.9 || N₂H₄(l) | 50.6 || N₂H₄(g) | 95.4 || N₂O(g) | 81.6 || NO(g) | 91.3 || N₂O₄(g) | 9.16 || N₂O₄(l) | 9.16 || H₂(g) | 0.0 || H₂O₂(g) | -136.3 || H₂O(g) | -241.8 || H₂O(l) | -285.8 |#### Part ACalculate \( \Delta H_\text{rxn} \) for the given chemical reaction using the standard enthalpies of formation from the table.- **Instructions:** Express your answer in kilojoules to one decimal place.\[ \Delta H_\text{rxn} = \]- **Feedback:** There is an option to provide feedback on your calculation.---To calculate \( \Delta H_\text{rxn} \), apply the formula:\[ \Delta H_\text{rxn} = \sum \Delta H_f^\circ \text{(products)} - \sum \Delta H_f^\circ \text{(reactants)} \] Substitute the appropriate values from the table to determine the reaction's

Answered: Image /qna-images/answer/6ddb9f68-04c9-4d1c-a4c7-6da9a9f5b5ad.jpg

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. Hydrazine (N₂H₁) is a fuel used by some spacecraft. It is normally oxidized by N₂O, according to the following equation: N₂H₁ (1) + N₂O₂(g) → 2N₂O(g) + 2H₂O(g) The table below shows standard enthalpies of formation for a number of substances. Substance AH; (kJ/mol) N₂(g) NH:(g) N₂H₁ (1) N₂H.(g) N₂O(g) NO(g) N₂O₁ (g) H₂O₂ (1) H₂O₂(g) H₂O(g) H₂O(1) 0.0 -45.9 50.6 95.4 81.6 91.3 9.16 -187.8 -136.3 -241.8 -285.8 Part A Calculate AHin for this reaction using standard enthalpies of formation from the table to the left. Express your answer in kilojoules to one decimal place. IVD ΑΣΦ AH = an Provide Feedback www. 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. Hydrazine (N₂H₁) is a fuel used by some spacecraft. It is normally oxidized by N₂O, according to the following equation: N₂H₁ (1) + N₂O₂(g) → 2N₂O(g) + 2H₂O(g) The table below shows standard enthalpies of formation for a number of substances. Substance AH; (kJ/mol) N₂(g) NH:(g) N₂H₁ (1) N₂H.(g) N₂O(g) NO(g) N₂O₁ (g) H₂O₂ (1) H₂O₂(g) H₂O(g) H₂O(1) 0.0 -45.9 50.6 95.4 81.6 91.3 9.16 -187.8 -136.3 -241.8 -285.8 Part A Calculate AHin for this reaction using standard enthalpies of formation from the table to the left. Express your answer in kilojoules to one decimal place. IVD ΑΣΦ AH = an Provide Feedback www. kJ

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

What is the enthalpy change when 2.00 mol of oxygen (O2) react? C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(l) ΔH = -5644 kJ
Question 5 of 26 Fill in the blanks: A substance having a mass 1.5 g is burned in a bomb calorimeter. The temperature started at 20.2 °C and leveled off at 23.5 °C. The manufacturer of the bomb calorimeter determined the heat capacity of the calorimeter to be 15.3 kJ/°C. Calculate the heat of combustion per gram of the given substance. Type your answer in whole number. kJ/g Answer:
They are all one question. In 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 60.42 grams of chromium to 98.12 °C and then drops it into a cup containing 82.86 grams of water at 23.37 °C. She measures the final temperature to be 28.57 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.80 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of chromium.Specific Heat (Cr) = ______J/g°C. In 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.Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is…
Suppose that the reaction of 4.739 moles produces 32.43 kJ of heat. What is the molar enthalpy of che reaction in kJ/mol? Report your answer to three decimal places (ignore significant figures).
Question 5 of 26 Fill in the blanks: A substance having a mass 1.5 g is burned in a bomb calorimeter. The temperature started at 20.2 °C and leveled off at 23.5 °C. The manufacturer of the bomb calorimeter determined the heat capacity of the calorimeter to be 15.3 kJ/°C. Calculate the heat of combustion per gram of the given substance. Type your answer in whole number. kJ/g Answer:
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
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
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.
A chemist burned a sample of coal in a bomb calorimeter. Her results are below. Calorimeter's Heat Capacity 7.264 kJ/°C Mass of Coal Initial Temperature Final Temperature 0.100 g 22.07°C 25.37°C The sample of coal that the chemist placed in the bomb was dry but when she finished the test there was a small amount of water in the bomb. Where did this water come from and how does it affect her result? The water came from the water surrounding the bomb so her measured heat of combustion is for a closed system. The water was a product of combustion so her measured heat of combustion is for an open system. The water came from the water surrounding the bomb so her measured heat of combustion is for an open system. The water was a product of combustion so her measured heat of combustion is for a closed system.
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?
The enthalpy of formation of H2O(l) is -285.8 kJ/mol. What is the enthalpy change if 1.62 g H2(g) reacts with 9.21 g O2(g) to form H2O(l)?
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.