[Referencea]The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is3AI(s) + 3NH, CIO, (s))Al, 0, (s) + AICI3(s) + 3NO(g) + 6H,0(g)Calculate AH for this reactionSubstance and State AH (kJ/mol)Al(s)Al, O3(s)AICI3 (s)H2O(g)NO(g)NH,CIO,(s)-1676-704242-90.-295AHkJ=

The enthalpy change is given by Here Enthalpy change of the reaction is the sum of heat of…

References] The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3Al(s) + 3NH4 CIO,(s) Al, 0, (s) + AICI (s) + 3NO(g) + 6H,O(g) Calculate AH for this reaction Substance and State AH (kJ/mol) Al(s) Al, O3(s) AICI (s) H20(g) NO(g) NH CIO (s) -1676 -704 -242 90. -295 AH kJ

References] The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3Al(s) + 3NH4 CIO,(s) Al, 0, (s) + AICI (s) + 3NO(g) + 6H,O(g) Calculate AH for this reaction Substance and State AH (kJ/mol) Al(s) Al, O3(s) AICI (s) H20(g) NO(g) NH CIO (s) -1676 -704 -242 90. -295 AH kJ

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...

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When 3.50 g of CH3OCH3 is burned at constant Pressure, 110.6 kJ of heat is given off. What is AH for this reaction? CH3OCH3 (1) + 302 (g) --> 2CO3 (s) +3H20 (s) AH xn = ? O 462 kJ/mole rxn O - 127 kJ/mole rxn O 2.61 kJ/mole rxn O -3480 kJ/mole rxn O - 7.16 kJ/mole rxn O -1460 kJ/mole rxn O -643 kJ/mole rxn O - 27.7 kJ/mole rxn
6 8 7. Consider the following reaction: 2 CH;OH (g) → 2 CH4() O2 (g), AH = + 252.8 kJ a) Is this reaction exothermic or endothermic? b) Calculate the amount of heat transferred when 26.0 g of CH3OH(g) is decomposed by this reaction at constant pressure. Express the heat to three significant digits with the appropriate units. c) For a given sample of CH;OH, the enthalpy change during the reaction is 82.9 kJ. What mass of methane gas is produced? Express the mass to three significant digits with the appropriate units. d) How many kilojoules of heat are released when 38.8 g CH4(g) reacts completely with 02(g) to form CH,OH(g) at constant pressure?
The standard state of carbon is graphite. ΔH°f,diamond is +1.896 kJ/mol. Diamonds are normally weighed in units of carats, where 1 carat = 0.200 g Determine the standard enthalpy of the reaction for the conversion of a 3.61 -carat diamond into an equivalent mass of graphite.
A chemist measures the energy change AH during the following reaction: 2 Fe₂O3(s) 4 FeO(s) + O₂(g) 1 AH 560, kJ Use the information to answer the following questions. This reaction is... Suppose 25.9 g of Fe₂O3 react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Be sure your answer has the correct number of significant digits. endothermic exothermic OYes, absorbed. Yes, released. No. 0... X G
In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe,O3(s) + 3CO(g) 2Fe(s) + 3CO,(g) AH° = - 28 kJ 3Fc,O3() + CO(g) 2Fe3O4() + CO,(g) AH = -59 kJ FezO4(s) + CO(g) 3FcO(s) + CO,(g) AH° = +38 kJ to calculate AH° for the reaction FeO() + CO(g) Fe(s) + CO2(g) AH° = i kJ
[2] When 1.045 g of CaO is added to 50.0 ml of water at 22.0 °C in a coffee-cup calorimeter, the temperature of the water increases to 29.3 °C. Assume that the specific heat and density of the solution is 4.184 J/g-°C and 1.00g/ml, respectively. The heat capacity of the calorimeter is 18.0 J/°C. Calculate AH for the reaction. CaO(s) + H2O(1) –→ Ca(OH)2(aq); AH =
MISSED THIS? Read Section 7.6 (Pages 281- 284), Watch IWE 7.7 View Available Hint(s) Nitromethane (CH,NO2) burns in air to produce significant amounts of heat via the following reaction Hint 1. Calculate the number of moles of nitromethane 2CH,NO, (1) +O2(g)→ 2CO2(g) +3H,O(1) + N2(g) The value of AH is related to the balanced chemical equation by the number of moles of nitromethane. Calculate the number of moles of nitromethane in a 2.73-kg sample. AHn -1418 kJ Express your answer in moles. mol CH, NO2 44.72 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Convert the mass of nitromethane from kg to g. Then use the molar mass of nitromethane as a conversion factor to obtain a value in mol HA Value Units = b
A chemist measures the energy change AH during the following reaction: 2 NH;(g) - N(9)+3H,(9) AH=160, kJ Use the information to answer the following questions. O endothermic. This reaction is... O exothermic. Suppose 93.6 g of NH, react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? O No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. Explanation Check 02021 McGraw Hill LLC. Al Rights Reserved Terms of Use Pivecy
How many moles of butane, C4H10(l), must be burned to produce 234 kJ of heat under standard state conditions? (The heat of combustion for butane is −2855.7 kJ/mol.)
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (C6H-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 14.00 °C to 33.17 °C over a time of 6.8 minutes. Next, 4.040 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 14.00 °C to 39.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about 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 the second experiment. Calculate the reaction enthalpy ΔΗ, per mole of…
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…
Using the provided table and the equation below, determine the heat of formation (in kJ/mol) for PbS. 2 PbS (s) + 3 O₂ (g) → 2 SO₂ (g) + 2 PbO (s) AH° = -828.4 kJ/mol Substance O₂ (g) SO: (g) PbO (S) AHf (kJ/mol) 0 -296.9 -217.3