### 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

Similar questions

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs
In an industrial process to produce ammonia (NH3); nitrogen, N2, reacts with hydrogen, H2, the enthalpy change (∆H) is – 46 kJ/mol. Write a correctly balanced equation for this reaction. Would this reaction absorb heat or give out heat to the environment?
A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g 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. Given that 156.61 g of solution increased in temperature by 4.82 °C, what quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g• °C.
13. Determine the amount of heat (in kJ) given off when 320 g of NO, are produced according to the equation: 2 NO(g) + 0,(g) 2 NO,(g) ΔΗ - -114.6 kJ/mol (Molar mass of NO, = 46 g/mol) * -1.49 x 10+2 -6.48 x 10+2 -3.99 x 10+2 O -2.74 x 10*2 -5.23 x 10+2 If th
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…
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?
Consider the following reaction. N2 + 3 H2 -> 2 NH3 ΔH = -92 kJ/mol If 35 g of NH3 are produced, then what amount of heat energy is released?
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
How much heat is released during the combustion of 7.50 g of methane (molar mass = 16.0 g/mol)?
AH° = -1670 kJ/mol 2. For this unbalanced chemical reaction: X(s) + 3/2 Y2(g) → X₂Y3 (S) 1. Calculate the mass in kg unit of X(s) that reacted with excess amount of Y₂ when 5650 kJ of heat is evolved. (A.W. for X and Y is equal 27 and 16 g/mol, respectively? 2. Explain, if the reaction is endothermic or not?
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?