10) Use enthalpy of formation to calculate the heat of the following reactions. Write the thermochemical equation (the chemical equation with energy included). (I) Answer: image | video a) H H H-C=C-H 52.47kJ/mol + Cl - Cl →> C =C OkJ/mol \ -117kJ/mol Cl Cl b) The synthesis of ammonia (nitrogen trihydride) from nitrogen and hydrogen. NH3 (g) is -45.9kJ/mol N2 (g) and H2 (g) are both OkJ/mol

10) Use enthalpy of formation to calculate the heat of the following reactions. Write the thermochemical equation (the chemical equation with energy included). (I) Answer: image | video a) H H H-C=C-H 52.47kJ/mol + Cl - Cl →> C =C OkJ/mol \ -117kJ/mol Cl Cl b) The synthesis of ammonia (nitrogen trihydride) from nitrogen and hydrogen. NH3 (g) is -45.9kJ/mol N2 (g) and H2 (g) are both OkJ/mol

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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2. Compute the heat of the formation of methane, CH4. The equation intricate is C (s) + 2 H2 (g) CH4 (g) AH = ? The thermochemical equations for the combustion are; (a) CH4 (g) + 2 02 (g)- CO2 (g) + 2H2O (1) AH = - 890.4 kJ (b) 2 H2 (g) + 02 (g) - 2H20 (1) AH = - 571.5 kJ (c) C (s) + 02 (g) -> CO2 (g) AH=-393 7 k.T
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Be sure to answer all parts. A 0.2975−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 2.437°C. (a) Calculate the heat associated with the burning Mg in kJ/g. kJ/g (b) Calculate the heat associated with the burning of Mg in kJ/mol.
A 148 g sample of an unknown metal at 74.0 oC is placed in a beaker containing 80.0 g of H2O at 25 oC. The final temperature of the metal sample and water is 32 oC. cH2O(l) = 4.184 j/ g oC SHOW ALL WORK (a) What is the specific heat (c) of the metal? (b) 5 common metals have the following specific heat capacities (c) [given in units of J/g oC] : Aluminum: 0.921 Copper: 0.377 Gold: 0.126 Iron: 0.461 Nickel: 0.502 Your sample is most likely to be which metal?
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) ΔH = -3352 kJ How much heat is released when 12.1 g of Al react with O2(g) at 25 oC and 1 atm? Group of answer choices A.) -3.59 × 105 kJ B.) -104 kJ C.) -1.50 × 103 kJ D.) -376 kJ
Please send me the question in 20 minutes it's very urgent plz
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s), ΔH = -1652 kJ (a) How much heat is released when 4.47 mol iron is reacted with excess O2?
Glucose, C6H12O6(s), (ΔHr° = -1275.2kJ/mol ) is converted to ethyl alcohol, C2H5OH(l), and carbon dioxide in the fermentation of grape juice. What quantity of heat is liberated when 750.0 mL of wine containing 12.0% ethyl alcohol by volume (d = 0.789g/cm3 ) are produced by the fermentation of grapejuice?
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,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 insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °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,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
O THERMOCHEMISTRY Using Hess's Law to calculate net reaction enthalpy Lindsay Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) → CH;OH(1) + H,0(1) AH=-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH;OCH,(g) + H,0(1) AH=8. kJ Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. II
The combustion of a sample of isoctane vapor at constant pressure raises the temperature of a calorimeter and its contents by 0.400 °C. The heat capacity of the calorimeter and water combined is 2.48 kJ/°C. How much heat was produced from the combustion? (variations of formula: c=q/mat)