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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A mass of 0.395 g of CHalg) is combusted in a bomb calorimeter that has a heat capacity of 785 C and contains 1.345 kg of water. If the temperature of the water in the calorimeter rises from 19.50°C to 28,50 C, what is energy of combustion of CH in k/mol? (Cwater4.184 J/gC) -289 k/mol 75.77x10klimol 544x10 kJ/mol 6-146klimol -234x 10 kmal
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(a) John performed a bomb calorimetry experiment using 2.147 g of CSH10O5. The temperature of the calorimeter rose from 24.18°C to 28.33°C. Given the heat capacity of the calorimeter and contents was 4.567 kJ/°C, determine the heat of combustion of C3H10O5 in kilojoule per mole.