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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Given the standard heats of formation for the following compounds, calculate the ΔH° heat of reaction, for the following reaction:
Fe3O4(s) + CO(g) ---> 3 FeO(s) + CO2(g)
ΔHf° for Fe3O4 = -1118 kJ
ΔHf° for CO = -110.5 kJ
ΔHf° for FeO = -272 kJ
ΔHf° for CO2 = -393.5 kJ
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- Using the provided enthalpy of formation, determine the enthalpy for the reaction: 3A (s)+ 2B (I) ->C (I) + 4D(s) substance AH;° (KJ/mol) A (s) -286arrow_forward1. 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)arrow_forwardGiven the heat of formation of the following compounds: CO2(g) ΔfH° = -393.5 kJ/mol H2O(l) ΔfH° = -285.9 kJ/mol CH3OH(l) ΔfH° = -238.6 kJ/mol What is the value of ΔrH° for the reaction: CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(l)arrow_forward
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