The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together.2A(s)+ FezO3(s) → 2Fe(s) + Al2Og(s)AH= -850. kJWhat mass of iron is formed when 589. kJ of heat are released ?O 56.0 gO 65.0 g0 61.6 gO 77.4gO 98.2 g« PreviousQuiz saved at 7:49amMacBook Air8068F6F7F4F5escF2F3F1%24245# 3aries are

Heat released and absorbed in a chemical reaction is function of the numbe of moles of reactants…

The highly exothermic thermite reaction, in which aluminum reduces iron(ll) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2As) + FezO(s) → 2Fe(s) + Al,O3(s) AH -850, k What mass of iron is formed when 589, kJ of heat are released ? O 56.0 g O 65.0g O 61.6 g O 774g O 98.2 8 • Previous

The highly exothermic thermite reaction, in which aluminum reduces iron(ll) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2As) + FezO(s) → 2Fe(s) + Al,O3(s) AH -850, k What mass of iron is formed when 589, kJ of heat are released ? O 56.0 g O 65.0g O 61.6 g O 774g O 98.2 8 • Previous

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

A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g 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. What is the total mass inside the calorimeter in grams?
A reaction between Mg and aqueous hydrochloric acid was performed to determine the heat of the reaction. A calorimeter with a heat capacity of 6.5 J/K was used. To the calorimeter 50.0 mL of 1.0 M HCI was added, the initial temperature was recorded and then 0.250 g of magnesium metal was added. The final temperature was then recorded. (Assume density of the solution is 1.03 g/mL; q = MCAT ; molar mass Mg = 24.31 g/mol; specific heat capacity of water = 4.184 J/g.K; q calorimeter = heat capacity x AT). The following data was recorded:Initial temperature:21.5°c ; Final Temperature: 45.1°c Calculate calorimeter (J) q solution (J) total amount of heat released (J), mol Mg, enthalpy of reaction in kJ/molor (q total/mol Mg). Just put the numerical values since units are already indicated. For the question, amount of heat released, there is no need to put the negative sign.
3. How many kilojoules are given off when 17.8 mol of CH₂(g) react? CH4(g) + 20₂(g) → CO₂(g) + 2H₂O(l) AH = -890.1 kJ
Consider the reaction, C2H4(g) + H2(g) → C2H6(g), where ΔH = –137 kJ. How many kilojoules are released when 3.5 mol of C2H4 reacts?
22.9 mL of an unknown acid was neutralized by mixing it with 50.3 mL of NaOH in an aqueous solution. The final temperature of the solution was 35.2 °C. The initial temperature of the acid and base was 22.0 °C. Assuming that the density of the solution is 1.00 g/mL and the specific heat is 4.184 J/g°C, what is the heat of neutralization reaction?
In the following reaction, what is the quantity of heat (in kJ) released when 3.91 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO₂ (g) + 2 H₂O(g) AH° = -802 kJ/mol -
A 8.27 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g 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. If -3.19 x 103 J of heat was lost during the dissolution reaction of 0.0708 moles of the unknown salt, what is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
4. You wish to determine the amount of heat produced by the reaction of propane with oxygen. You are given some known reactions: I. II. III. 3 C(s) (g) + 4H₂(g) → C₂H₂ (g) C(s) (g) + O₂(g) → CO₂ (g) H₂(g) + O₂(g) → H₂O (1) ΔΗ, ΔΗ, ΔΗ, (a) Combine reactions 1, 2 and 3 to form a series of steps that sum to the combustion of propane: C₂H₂(g) +50₂ (g) →3CO₂ (g) + 4H₂O (1) (b) Given the following values for the enthalpy changes, combustion of propane. AH₂=-393.5 kJ/mol AH, =-103.85 kJ/mol calculate AH for the AH, = -285.8kJ/mol
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. What is the total heat for the dissolution reaction of the 6.61 g of salt
If 2C4H10 + 13O2 --> 8CO2 + 1OH2O is exothermic, is energy (heat) a reactant or product?
48.2 mL of a solution of HCl is combined with 110.7 mL of 1.35 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C, and the final temperature after reaction is 29.3°C. What is the molarity of the HCl solution? You may assume that there is an excess of base (so that all the HCI has reacted), that the specific heat of the reaction mixture is 0.96 cal/g °C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mole.
In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.81 °C to 28.58 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH= kJ/mol H₂O