### Reaction and Heat Release Calculation**Chemical Reaction:**\[ 2X + Y_2Z_3 \rightarrow 2Y + X_2Z_3 \]**Change in Enthalpy (\(\Delta H\)):** \[ \Delta H = -325 \, \text{kJ/mol} \]**Problem Statement:**Given the equation above, determine **how many kilojoules of heat are released** when 2.09 moles of Y are created.**Calculation Steps:** To find the heat released when 2.09 moles of Y are produced, given that the reaction produces 2 moles of Y and releases 325 kJ of heat:1. First, note that the production of 2 moles of Y releases 325 kJ.2. Calculate the heat released per mole of Y: \[ \text{Heat per mole of } Y = \frac{325 \, \text{kJ}}{2} \]3. Multiply this value by 2.09 to find the total heat released for 2.09 moles of Y.This will give you the amount of heat released in kilojoules.

Given that: 2X + Y2Z3 -----> 2Y + X2Z3 ∆H = -325 kJ/mol

Answered: 2 X+ Y2Z3 →2 Y+ X2Z3, AH = -325 kJ/mol…

2 X+ Y2Z3 →2 Y+ X2Z3, AH = -325 kJ/mol Given the equation above how many kilojoules of heat are released when 2.09 moles of Y are created?

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: use the photo attached please to answer the questions 1. This reaction is... 2.Suppose 56.0g of…

A: If the heat is released reaction is exothermic and if the heat is being absorbed the reaction is…

Q: What is the final temperature of a 56 g sample of water if the initial temperature was 4.0°C and it…

A: Given: Mass, m = 56 g Heat, q = 3046 J Specific heat of water, c = 4.184 Initial temperature, Ti =…

Q: Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor.…

A: Combustion is the reaction of a substance with oxygen. In the presence of oxygen, hydrocarbons…

Q: The heat equation, as given in the introduction, can also be rearranged to calculate the mass or…

A: The specific heat required to raise the temperature of a substance is given as:

Q: When 3 moles of C is formed, what is the change in enthalpy? 3A + 6B + 5 kJ → 2C

A: Answer given below

Q: The temperature of 756 g of water in a calorimeterincreases from 23.2°C to 37.6°C. How much heat…

A: Given: Mass = 756g Initial temperature= 23.2oC Final temperature= 37.6oC To find: The heat given off…

Q: Benzene is burned in oxygen. Write the balanced chemical question. Calculate the change in heat of…

A: Given ,Benzene is burned in oxygen.Objective :Write the balanced chemical equation.Calculate heat of…

Q: If 63.50 g of an unknown metal at 97.6 °C initially produced a resulting temperature of 39.5 °C when…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 2 moles of potassium metal reacts with liquid water to produce solid potassium hydroxide, hydrogen…

A: 2K + 2H2O →2KOH + H2 Given that ∆H = - 162.4 kJ/mol For 2 mol of potassium metal (K) , ∆H = 2 mol x…

Q: A reaction is performed in water inside of a calorimeter. The mass of solution inside the…

Q: Using the enthalpy change of -1594 kJ, what is the amount of heat absorbed or released when 1.10 L…

Q: Propane, C3H8(g), is used in many instances to produce heat by burning: C3H8(g) + 5O2(g) → 3CO2(g)…

A: Given :- C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH = -2220. kJ To calculate :- Mass of O2…

Q: You performed the displayed reaction in the lab and determined that 336.74 J of heat was released.…

A: The given chemical reaction that has been carried out is given by: NCl3(g) + 3H2 (g) ——> NH3 (g)…

Q: If the heat of combustion for a specific compound is-1190.0 kJ/mol and its molar mass is 63.57…

A: Heat of combustion: The enthalpy of combustion is the enthalpy change that occurs when 1 mole of a…

Q: 8. How much heat is released when 266g of carbon dioxide are formed? 2C₂H +70, 4CO₂ + 6H₂O -> AH =…

A: 1.Combusion of ethane is exothermic reaction. 2 . when etane undergo combusion give carbon…

Q: 100 g of a solution (specific heat of 0.32 J/g C) undergoes a reaction in which 74.84 J of heat is…

A: Mass of solution = 100 g Specific heat = 0.32 J/g oC Heat released = 74.84 J

Q: A student performed the procedure described in the lab manual using 49.9 mL of 1.0 M HCI and 49.3 mL…

A: Molarity of HCl = 1.0 MVolume of HCl: 49.9 mLMolarity of NaOH = 1.0 MVolume of NaOH = 49.3 mLInitial…

Q: Using the equations 2 Fe (s) + 3 C2 (g) → 2 FECI3 (s) AH° = -800.0 kJ/mol Si(s) + 2 Cl2 (g) → SiCl,…

A: 2Fe (s) + 3Cl2 (g) -------> 2FeCl3 (s) ∆ H1° = -800.0 kJ/mol ...................(1) Si (s)…

Q: Calorimetry measures the heat transfer for chemical reactions. Find two foods n your house that you…

A: Mass of food = 2 g Volume = 5L

Q: How many grams of carbon are present if it requires 57.5 kJ of energy to heat a sample from 20.0 to…

Q: A student heats 62.33 grams of chromium to 99.36 °C and then drops it into a cup containing 82.16…

A: Given, mass of chromium =62.33 graminitial temperature of chromium =99.36 °Cmass of water =82.16…

Q: A sample of 35.41 g of Cus at 96.73 degrees celcius was added to a calorimeter containing 148.3 g of…

A: Given:…

Q: An unknown mass of sand and water at 23 °C each absorb 1.95 × 10³ J of heat. The final temperature…

A: Given: Amount of heat absorbed = 1950 J Initial temperature of sand and water = 23 oC Final…

Q: The temperature of a 33.7 g sample of metal increases by 27.2°C after absorbing 201.7 J of heat.…

A: Interpretation: The temperature of a 33.7 g sample of metal increases by 27.2°C after absorbing…

Q: The heat change that accompanies the formation of 1.00 mol of carbon dioxide from its elements is…

A: we have to calculate the heat change for the formation of 0.650 mole of carbon dioxide

Q: Hydrogen sulfide is produced during the decomposition of organic matter. When 0.5380 mol H2S burns…

A: Given: H2S burns to produce SO2(g) and H2O(g) with heat release of -278.7 kJ

Q: 1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in…

A: The energy difference of the products and reactants is known as the energy change of a reaction.

Q: 4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be…

A: The amount of heat required to increase the temperature of the 1 g of the substance by 1 degree is…

Q: When a metal at a higher temperature is transferred to water at a lower temperature, heat the value…

A: Heat flows from hot object to cold object until they reach at same temperature. A calorimeter is…

Q: Calculate the change in energy for the following processes and identify if the process is…

Q: When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass =…

A: Iron reacts with chlorine to form iron(II) chloride. When 3.22 g of is formed, 6.8 kJ of heat is…

Q: If 87 J of heat are added to a balloon, causing it to expand from 1.0 L to 1.4 L under 0.97 atm of…

Q: The amount of energy needed to heat 2.00 grams of mercury from 50.00 to 90.00 is 11.28 Jules. The…

Question

100%

### Reaction and Heat Release Calculation

**Chemical Reaction:**

\[ 2X + Y_2Z_3 \rightarrow 2Y + X_2Z_3 \]

**Change in Enthalpy (\(\Delta H\)):**
\[ \Delta H = -325 \, \text{kJ/mol} \]

**Problem Statement:**

Given the equation above, determine **how many kilojoules of heat are released** when 2.09 moles of Y are created.

**Calculation Steps:**
To find the heat released when 2.09 moles of Y are produced, given that the reaction produces 2 moles of Y and releases 325 kJ of heat:

1. First, note that the production of 2 moles of Y releases 325 kJ.
2. Calculate the heat released per mole of Y:
\[ \text{Heat per mole of } Y = \frac{325 \, \text{kJ}}{2} \]
3. Multiply this value by 2.09 to find the total heat released for 2.09 moles of Y.

This will give you the amount of heat released in kilojoules.

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

In a simple calorimeter, a piece of metal weighing 48.67 g was heated to 120.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. Is this process endothermic or exothermic? Explain. Show Your Work
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
If it takes 41.72 joules of heat for a piece of gold weighing 18.69 grams from 10.0oC to 27.0oC, what is the specific heat of the gold?
The Law of Conservation of Energy states, when applied to Calorimetry, states that heat is neither lost nor generated, but merely changes form during processes. Which of these calorimetry equations corresponds to that law?
F HNO3 (1 mole) H2SO4, heat ?
If 585 J of energy are absorbed by 125.6 g of aluminum and the initial temperature is from 20.0 oC, what is the final temperature? Is this endothermic or exothermic?
A chunk of gold (specific heat: 0.126) initially at 82.2 ˚C is placed in 75.5 g of water (specific heat: 184) initially at 22.0 ˚C. After a short time, both the water and the gold are at 41.0 ˚C. What was the mass of the gold?
If 67.2 J of heat is added to a 24.6 g sample of silver, how much will the temperature increase by? The specific heat of silver is 0.235 J/goC.
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
2 moles of lithium metal reacts with liquid water to produce solid lithium hydroxide, hydrogen gas, and 402.4 kJ/mol of heat energy. a) write a balanced thermochemical equation for the reaction b) how much heat would be produced by the reaction of 14 g of lithium with an excess of liquid water c) is the reaction endothermic or exothermic?
4. 30.0 g of a substance (molar mass: 46 g/mo) required 262 J of heat to raise its temperature from 32.0°C to 37.4°C. What is the specific heat per gram and per mole of this substance?
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.