The thermite reaction is written below. Show that the heat released in this reaction is sufficient for the iron to be produced as molten metal. Find the enthalpy of formation of the overall reaction. Al(s) + Where: Al ΔΗ°F= 0 Al2.03 AH° -2076 Fe AHF 0 Fe2O3 AHF-745 Fe₂O3(s)→ Al₂O3(s) + Fe(1)

The thermite reaction is written below. Show that the heat released in this reaction is sufficient for the iron to be produced as molten metal. Find the enthalpy of formation of the overall reaction. Al(s) + Where: Al ΔΗ°F= 0 Al2.03 AH° -2076 Fe AHF 0 Fe2O3 AHF-745 Fe₂O3(s)→ Al₂O3(s) + Fe(1)

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

Given that: AH°F [Fe(OH)3 (s)] -- 823.0 kJ/mol AH°F [Fe+3 (aq)] = - 48.5 kJ/mol AH°F [OH (aq)] = - 230.0 kJ/mol What is the enthalpy change for the precipitation reaction of Fe(OH)3 (s)? O A-1101.5 kJ/mol O B.- 84.5 kJ/mol Oc-447.5 kJ/mo1 O D.- 1561.5 kJ/mol O E. - 544.5 kJ/mol
A student dissolves 11.5 g of ammonium nitrate (NH4NO3) in 200. g of water in a well-insulated open cup. She then observes the temperature of the water fall from 20.0 °C to 16.6 °C over the course of 4 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3(s) NH(aq) + NO, (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ AH per mole of…
A student dissolves 14.0 g of ammonium nitrate (NH4NO3) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0 °C to 16.6 °C over the course of 5.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO₂ (s) NH(aq) + NO3(aq) - You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AHxn per mole…
Item 22 22 of 25 I Review I Constants I Periodic Table Classify the following as exothermic or endothermic reactions and give AH for each. Part E Classify reaction as exothermic or endothermic. Formation of aluminum oxide and copper from aluminum and copper (II) oxide: 2Al(s)+3CuO(s)→Al2O3(s)+3Cu(s)+1204kJ exothermic reaction O endothermic reaction Part F Give AH for reaction above. Express your answer as an integer. ? kJ
The Sun supplies about 1.0 kilowatt of energy for each squaremeter of surface area (1.0 kW/m2, where a watt = 1 J/s).Plants produce the equivalent of about 0.20 g of sucrose(C12H22O11) per hour per square meter. Assuming that thesucrose is produced as follows, calculate the percentage ofsunlight used to produce sucrose.12 CO2(g)+ 11 H2O(l)-----> C12H22O11 + 12 O2(g)ΔH = 5645 kJ
1. How much energy in kJ is released when 124.49 g of nickel react with an excess of phosphorus? 5 Ni + 2 P -> Ni5P2 △ H = 436 kJ/mol 2.How much titanium in grams is required to release 538.13 kJ of heat? Ti + 2 B -> TiB2 △ H = 316 kJ/mol
Give detailed Solution
Given the overall reaction from the previous problem: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes: Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic? Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction. If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?
Explain step by step why each can or cannot occur.
1. How many kJ of energy are released by 34.65 g of boron? Ti + 2 B -> TiB2 △ H = 316 kJ/mol 2. How much energy in kJ is released when 14.17 g of aluminum react with an excess of copper oxide? 3 CuO + 2 Al -> 3 Cu + Al2O3 △ H = 1190 kJ/mol 3. If 36.26 grams of aluminum is heated from 18 oC to 26 oC how much energy was required? sAl = 0.897 J/(gK)
For a reaction with ΔHo = 40 kJ/mol, decide which of the following statements is (are) true. Correct any false statement to make it true. (a) The reaction is exothermic; (b) ΔGo for the reaction is positive; (c) Keq is greater than 1; (d) the bonds in the starting materials are stronger than the bonds in the product; and (e) the product is favored at equilibrium.
The reaction of CH3OH(g) with N2(g) to give HCN(g), NH3(g), and O2(g) requires 164 kJ/mol of CH3OH(g). Write a balanced chemical equation for this reaction. Include the phases of all species in the reaction. How much heat is involved in the reaction of 65.0 g of CH3OH(g) with excess N2(g) to give HCN(g) and NH3(g) in this reaction?