**Thermochemical Equation and Enthalpy Calculation**Given the following thermochemical equations:1. \( X_2 + 3Y_2 \rightarrow 2XY_3 \) \( \Delta H_1 = -380 \text{ kJ} \)2. \( X_2 + 2Z_2 \rightarrow 2XZ_2 \) \( \Delta H_2 = -120 \text{ kJ} \)3. \( 2Y_2 + Z_2 \rightarrow 2Y_2Z \) \( \Delta H_3 = -270 \text{ kJ} \)**Objective:**Calculate the change in enthalpy for the reaction:\[ 4XY_3 + 7Z_2 \rightarrow 6Y_2Z + 4XZ_2 \]### Explanation:#### Step-by-Step Approach:1. **Identify the Target Reaction:** \[ 4XY_3 + 7Z_2 \rightarrow 6Y_2Z + 4XZ_2 \] 2. **Express the Target Reaction using Given Equations:** By manipulating the given equations, try to arrive at the target reaction. Consider the following transformations and additions: Multiply the first equation by 2: \[ 2(X_2 + 3Y_2 \rightarrow 2XY_3) \] Simplifies to: \[ 2X_2 + 6Y_2 \rightarrow 4XY_3 \] \( \Delta H_1' = 2 \times -380 \text{ kJ} = -760 \text{ kJ} \) Using the third equation as it is: \[ 2Y_2 + Z_2 \rightarrow 2Y_2Z \] \( \Delta H_3 = -270 \text{ kJ} \) To match the required coefficients: By multiplying the third equation by 3: \[ 3(2Y_2 + Z_2 \rightarrow 2Y_2Z) \] Simplifies to: \[ 6Y_2 + 3Z_2 \rightarrow 6Y_2Z \] \( \Delta H_3' = 3 \times -270 \text{ kJ} = -810 \text{

It is based on the concept of enthalpy change of the reaction.Here we are required to find the…

Given the thermochemical equations X₂ + 3 Y₂ → 2XY3 X₂ +2Z₂ → 2XZ₂ AH₁ = -380 kJ AH₂ = -120 kJ 2Y₂+Z₂2Y₂Z AH3 = -270 kJ Calculate the change in enthalpy for the reaction. 4XY3 +7Z₂ →→ 6Y₂Z + 4 XZ₂

Given the thermochemical equations X₂ + 3 Y₂ → 2XY3 X₂ +2Z₂ → 2XZ₂ AH₁ = -380 kJ AH₂ = -120 kJ 2Y₂+Z₂2Y₂Z AH3 = -270 kJ Calculate the change in enthalpy for the reaction. 4XY3 +7Z₂ →→ 6Y₂Z + 4 XZ₂

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

Related questions

Q: Determine the mass of CO2CO2 produced by burning enough carbon (in the form of charcoal) to produce…

A: The balanced chemical reaction is C(s)+O2 (g)→CO2(g); ΔrH∘=−393.5 kJ-mol-1 The mass of CO2…

Q: From data found in appendix G, calculate the enthalpy of the following reaction: PH3(g) + 3 Cl2(g)…

A: Enthalpy is thermodynamics property which measure the energy of the reaction. Here we are required…

Q: A 100.0 g piece of metal at 100°C is placed in contact with 50.0 g of water (s = 4.184 J g–1 °C–1)…

Q: H₂SO4 reacts with NaOH to form water and Na2SO4. In a simple calorimeter, a 100.00 mL sample of…

A: Given,Molarity of H2SO4 = Volume of H2SO4 = Volume of NaOH = Total volume of solution Change in…

Q: Consider the following balanced thermochemical equation for a reaction sometimes used for H2S…

A: Given, 18S8(s) + H2(g) → H2S(g), ΔHrxn = −20.2 kJ18 mole of S8 sulphur react to…

Q: What is the heat capacity of mercury in J⋅mol−1⋅∘C−1?

Q: Given the thermochemical equations X, + 3 Y, → 2 XY, AH1 = -390 kJ X, +2 Z, → 2 XZ, AH2 = -160 kJ…

A: In-order to find the enthalpy change of the desired reaction, the given reactions has to be written.

Q: Sulfur dioxide gas reacts with oxygen to form sulfur trioxide in an exothermic reaction according…

A: Enthalpy of a reaction is the energy that liberated or consumed in the chemical reaction. For an…

Q: When 4.00 g of sodium hydrogen carbonate reacts completely with 90.0 ml of acetic acid, the…

A: The molar enthalpy of a reaction indicates the enthalpy change produced as a result of the formation…

Q: Calculate the value of ΔH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given…

A: Given Chemical equation Equation1 ,2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) ΔH = -87.2 kJ…

Q: thermometer A sample of polystyrene, which has a specific heat capacity of 1.880 J-g.°c, is put into…

A: Specific heat capacity: The amount of energy that is required to raise the temperature by 10 , of 1…

Q: - the AH value

Q: The Combustion of gasoline is an exothermic process. Let us assume that the combustion of gasoline…

A: In this question we want to determine the heat Produces from the combustion of 692g of Octane. How…

Q: Standard Enthalpy of Formation and Hess's Law 15. Consider the following data: ΔΗ° (kJ) -62.8 -635.5…

A: Hess's law describes that regardless of the multiple stages or steps of a reaction, the total…

Q: 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations:…

A: Solution

Q: Given the thermochemical equations X₂ +3Y₂ → 2XY, AH₁ = -310 kJ X₂ +22₂ → 2XZ₂ AH₂ = -160 kJ…

Q: Compounds of boron and hydrogen are remarkable for their unusual bonding and also for their…

A: The given reaction is, ΔHrxn = −755.4 kJ Total 7.313 Kg = 7313 g B2H6 is reacted. molar mass of…

Q: The following thermochemical equations are provided; C2H2 (g) + O2 (g) --> 2 CO2 (g) + H2O (l)…

A: According to Hess's law of thermodynamics, if a reaction proceeds through the multi-steps, then…

Q: Given the thermochemical equations X₂+3Y2 2XY, AH₁ = -380 kJ X₂+2Z2 → 2XZ₂ AH2 = -190 kJ 2Y2 +…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: Given the thermochemical equations X2+3Y2⟶2XY3Δ?1=−330 kJ X2+2Z2⟶2XZ2Δ?2=−190 kJ 2Y2+Z2⟶2Y2ZΔ?3=−220…

Q: Calculate the value of ΔH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given…

A: According to law of Laplace and Lavoisier: If any thermochemical balanced reaction is reversed, then…

Q: Measurements show that the energy of a mixture of gaseous reactants increases by 369. kJ during a…

A: We have to calculate the change in enthalpy and nature of reaction.

Q: From the thermochemical equations given below, and applying Hess’s law, NO(g) + O3(g)= NO2(g) + O2…

Q: 7N2(9) +5H2(9) → NH3(g) AH = -46KJ z H2c9) +Clz@) → HCl) N2(9) +4H2(9) + Cl29) → 2NH¼C\(s) → HCl(g)…

Q: A 27.24 g27.24 g sample of a substance is initially at 26.6 ∘C26.6 ∘C . After absorbing 496 cal496…

Q: A₂H.(g) + 6 X₂(g) → 2 AX,(g) + 6 HX(g) A and X are unknown elements. When the reaction given above…

Q: A piece of metal weighing 5.10 gg at a temperature of 48.5 ∘C∘C was placed in a calorimeter in…

Q: Calculate the value of ΔH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given…

A: The enthalpy of reaction of given equation can be find using Hess's law of thermodynamics.…

Q: which is the correct enthalpy of formation reaction for nitrogen monoxide gas?

Q: Given the standard enthalpies of formation for the following substances, determine the reaction…

A: Interpretation - To determine the enthalpy of reaction when here standard enthalpies of formation…

Q: Given the thermochemical equations X2+3Y2⟶2XY3 Δ?1=−390 kJ X2+2Z2⟶2XZ2…

A: Given: (1) X2 + 3Y2⟶ 2XY3 .........1 Δ?1=−390 kJ (2) X2 + 2Z2⟶ 2XZ2 ...............2…

Q: ERMODYNAMICS: Given the following hypothetical thermochemical equations: 3 (g) + 3Q2X (g) → 4Q2 (g)…

Q: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (l)…

A: 2QJ3 (g) + 3Q2X (g) ---> 4Q2 (g) + 3J2X (l) ΔH = -1074.4 kJ 4QJ3 (g) + 3X2 (g)…

Q: When 2.25 grams of zinc reacts with 75.0 mL of 0.500 M HCl(aq), 5.63 kJ of heat are produced.…

A: The given data - The mass of Zinc = 2.25 The volume of HCl = 75.0 mL The molarity of the HCl = 0.500…

Q: Use the balanced thermochemical equations shown below (reactions 1,2, & 3) to determine the enthalpy…

A: Solid magnesium react with oxygen and produced solid magnesium oxide

Q: H2O(g)is −241.82kJ/mol The standard enthalpy of formation for CO2(g)is −393.5kJ/mol The standard…

A: Given data is The standard enthalpy of formation for H2O (g)is −241.82 kJ/mol The standard enthalpy…

Q: Given the thermochemical equations X, + 3 Y, → 2XY, ΔΗ = -390 kJ - X, + 2Z, – 2 XZ, AH2 = -120 kJ…

Q: Given the thermochemical equations X₂ + 3Y₂ → ->> 2XY, X₂ +2Z₂ → 2XZ₂ ΔΗ, = -160 kJ 2Y₂+Z₂2Y₂Z AH3 =…

A: Given, a) X2 + 3 Y2 -----> 2 XY3 ∆H1 = -320 kJ b) X2 + 2 Z2 -----> 2 XZ2 ∆H2 = -160 kJ c) 2…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.27 kg sample…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.59 kg sample…

Q: Given the thermochemical equation 2A+B⟶3C+DΔ?=293 kJ determine the enthalpy change, Δ?,ΔH, for…

Q: Given the thermochemical equations X2+3Y2⟶2XY3 ΔH1=−390 kJ X2+2Z2⟶2XZ2 ΔH2=−120 kJ 2Y2+Z2⟶2Y2Z…

Q: THIS QUESTION MUST BE COMPLETED Solid potassium nitrate dissolves in water according to the equation…

A: Answer: Heat absorbed by the solute during dissolution would cause the decrease in temperature of…

Q: What mass of natural gas (CH4) must burn to emit 265 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)…

A: To solve this problem we have to consider the given thermochemical equation . According to this…

Question

**Thermochemical Equation and Enthalpy Calculation**

Given the following thermochemical equations:

1. \( X_2 + 3Y_2 \rightarrow 2XY_3 \) \( \Delta H_1 = -380 \text{ kJ} \)
2. \( X_2 + 2Z_2 \rightarrow 2XZ_2 \) \( \Delta H_2 = -120 \text{ kJ} \)
3. \( 2Y_2 + Z_2 \rightarrow 2Y_2Z \) \( \Delta H_3 = -270 \text{ kJ} \)

**Objective:**
Calculate the change in enthalpy for the reaction:

\[ 4XY_3 + 7Z_2 \rightarrow 6Y_2Z + 4XZ_2 \]

### Explanation:

#### Step-by-Step Approach:

1. **Identify the Target Reaction:**
\[ 4XY_3 + 7Z_2 \rightarrow 6Y_2Z + 4XZ_2 \]

2. **Express the Target Reaction using Given Equations:**

By manipulating the given equations, try to arrive at the target reaction. Consider the following transformations and additions:

Multiply the first equation by 2:
\[ 2(X_2 + 3Y_2 \rightarrow 2XY_3) \]
Simplifies to:
\[ 2X_2 + 6Y_2 \rightarrow 4XY_3 \] \( \Delta H_1' = 2 \times -380 \text{ kJ} = -760 \text{ kJ} \)

Using the third equation as it is:
\[ 2Y_2 + Z_2 \rightarrow 2Y_2Z \] \( \Delta H_3 = -270 \text{ kJ} \)

To match the required coefficients:
By multiplying the third equation by 3:
\[ 3(2Y_2 + Z_2 \rightarrow 2Y_2Z) \]
Simplifies to:
\[ 6Y_2 + 3Z_2 \rightarrow 6Y_2Z \] \( \Delta H_3' = 3 \times -270 \text{ kJ} = -810 \text{

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Given data

VIEW

Step 2: introduction to enthalpy

VIEW

Step 3: Finding the change in the enthalpy of the reaction

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 19 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Given the thermochemical equations X2+3Y2⟶2XY3. Δ?1=−340 kJ X2+2Z2⟶2XZ2 Δ?2=−190 kJ 2Y2+Z2⟶2Y2Z Δ?3=−250 kJ Calculate the change in enthalpy for the reaction. 4 XY3+7 Z2⟶6 Y2Z+4 XZ2
Given the thermochemical equations X, + 3 Y, 2XY3 AH1 = -380 kJ > 2. X, + 2Z, → 2 XZ, ΔΗ = -110 kJ 2 Y, + Z, → 2 Y,Z AH3 = -280 kJ Calculate the change in enthalpy for the reaction. 4 XY, + 7Z, 6 Y,Z + 4 XZ, 3 ΔΗ kJ
Given the balanced thermochemical reaction shown below, assuming enough of both reactants are present, how many grams of H2O will be produced if 6,474 kJ of heat is produced? Assume that the reaction goes to 100% completion. 2 C6H14 (g) + 19 O2 (g) →→ 12 CO2 (g) + 14 H2O (g) \DeltaΔH = -7756 kJ Report your answer to one decimal place with no units. Do NOT use scientific notation.
100 g of hot metal was put in 222.2 g of water in a container. Both the container and the water are at 20 deg C. Cp of water is 4.184 J K−1 g −1 and Cp of metal is 0.4444 J K−1 g −1. 2.222 kJ K−1 is the heat capacity of the container. 22 C is the final temperature of the metal, water and the container. Determine the initial temperature of the metal.
A sample of 3.20 g of calcium hydroxide, Ca(OH)2(s) is added to 90.0 mL of dilute hydrochloric acid in a calorimeter. The temperature goes from 22.4°C to 24.7°C. Calculate the molar enthalpy of the reaction?
Given the thermochemical equations X, + 3 Y, → 2XY, AH1 = -390 kJ X, + 2Z, → 2XZ, AH2 = -120 kJ %3D 2 Y2 + Z, → 2 Y,Z AH3 = -250 kJ %3D | Calculate the change in enthalpy for the reaction. 4 XY, + 7Z, → 6 Y,Z + 4 XZ, AH =
Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = −1036 kJ Calculate the enthalpy change to burn 30.5 g of hydrogen sulfide. kJ
Use standard enthalpies of formation to determine ΔHorxn for: 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) Enter in kJ.
Given the following thermochemical equations, 2Cu (s) + S (s) · → Cu₂S (s) AH° = -79.5 kJ S (s) + O₂ (g) → SO₂ (g) AH° = −297 kJ Cu₂ S (s) +20₂ (g) → 2CuO (s) + SO₂ (g) AH° = -527.5 kJ calculate the standard enthalpy of formation (in kJ mole¹¹) of CuO (s).
2 H2O2(l) → 2 H2O(l) + O2(g) Δ Hrxn = −196.1 kJ Calculate the heat for the decomposition of 599 kg of H2O2.
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (I) AH = -1,089.5 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (I) AH = -1,502 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
Determine the change in enthalpy for the following reaction:SnO2(s) + 2 H2(g) → Sn(s) + 2 H2O(l)∆Hac,SnO2(s) = -1381.1 kJ/molrxn ∆Hac,Sn(s) = -302.1 kJ/molrxn∆Hac,H2(g) = -435.3 kJ/molrxn ∆Hac,H2O(l) = -970.3 kJ/molrxn