are reacted?to0o loD. Consider the following reaction:2H,(g) + O,(g)AH = -572 kJ-%3Da. How much heat is evolved for the production of1.00 mole of H;O(1)?b. How much heat is evolved when 4.03 g hydrogen arereacted with excess oxygen?w to olgmsa-0.0E A.02c. How much heat is evolved when 186 g oxygen are reactedwith excess hydrogen?edd. The total volume of hydrogen gas needed to fill the Hin-denburg was 2.0 × 10* L at 1.0 atm and 25°C. How muchheat was evolved when the Hindenburg exploded, assum-ing all of the hydrogen reacted?E HonST o bobl-51. Consider the combustion of propane:2isllsq muniule to olgme

"Since there are multiple sub-parts in this question and it is not mentioned that which one has to…

D. Consider the following reaction: 2H,(g) + O,(g) –→ 2H,0(1) AH = -572 kJ %3D - a. How much heat is evolved for the production of 1.00 mole of H,O(1)? b. How much heat is evolved when 4.03 g hydrogen are reacted with excess oxygen? wto olgmsa -0.08 A 02- c. How much heat is evolved when 186 g oxygen are reacted with excess hydrogen?

D. Consider the following reaction: 2H,(g) + O,(g) –→ 2H,0(1) AH = -572 kJ %3D - a. How much heat is evolved for the production of 1.00 mole of H,O(1)? b. How much heat is evolved when 4.03 g hydrogen are reacted with excess oxygen? wto olgmsa -0.08 A 02- c. How much heat is evolved when 186 g oxygen are reacted with excess hydrogen?

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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( is the answer is + 46.48 or -46.48 plzz telll ...why + or why - also explain
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Pls help ASAP. Pls show all work.
18. Calculate the heat of reaction at constant volume for 5.00 g C3H8 ,considering the following chemical reaction: C3H8 (g) + O2(g) --------------------> CO2 (g) + H2O (g) heat of standard formation: O2 = 0.00 kJ / mole, H2O (g) = -245 kJ / mole, CO2 = -318 kJ/mole and C3H8 = -438 kJ / mole C3H8 = 44.09 g/mole Temperature is 33 oC a. -789 kJ b. -212 kJ c. 412 kJ d. -169 kJ
0. Calculate the heat change, in kJ, if 5.9217x1014 ng of phosphorus pentachloride were produced in the following reaction: PC13(g) + C2(g) → PCl:(g) AH°{ = -84.2 kJ/mol %3D
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The thermite reaction is a very exothermic reaction; it has been used to produce liquid iron for welding. A mixture of 2 mol of powdered aluminum metal and 1 mol of iron(III) oxide yields liquid iron and solid aluminum oxide. How many grams of the mixture are needed to produce 219 k) of heat? Data: AH;(Al(s)) = 0 kJ/mol AH (Fe,O3 (s)) = -825.5 kJ/mol AH (Fe(1)) = 12.4 kJ/mol AH;(Al2O3 (s)) = -1675.7 kJ/mol
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