1
answer
0
watching
533
views
19 Nov 2019
What is the change in the internal energy of a system (delta U) if 71 kJ of heat energy is absorbed by the system and 12 kJ of work is performed on system? Write a balanced thermochemical equation for the following process: If 2 mol of sodium metal reacts with 1 mol of fluorine gas at constant pressure, 2 mol of solid sodium fluoride is produced and 409.2kJ of heat is released. How much energy is released if one mole of sodium fluoride is produced? A gallon of water was heated from room temperature. 25 degree C, to almost boiling. 97 degree C. How much energy did the water absorb during this process? Given the thermochemical equation: 2Al(s) + 3/2 O_2(g) rightarrow Al_2O_3(s): delta H = -1, 676 kJ determine delta H for the following reaction: 2Al_2O_3(s) rightarrow 4Al(s) + 3O_2(g) Given the thermochemical reactions, calculate delta H for Na(s) + 1/2 Cl_2(g) rightarrow Na(g) + Cl(g): delta H = 230.0 kJ Na(s) + 1/2 Cl_2(g) rightarrow Nacl(s): delta H =-411 kJ Na(g) + Cl(g) rightarrow NaCI(s) Given the thermochemical reactions, calculate delta H of solid iron (III) bromide from the elements. Fe(s) + Br_2(l) rightarrow FeBr_2(s): delta H = -249.8 kJ FeBr_3 (s) rightarrow FeBr_2(s) + 1/2 Br_2(l): delta H = 18.4 kJ
What is the change in the internal energy of a system (delta U) if 71 kJ of heat energy is absorbed by the system and 12 kJ of work is performed on system? Write a balanced thermochemical equation for the following process: If 2 mol of sodium metal reacts with 1 mol of fluorine gas at constant pressure, 2 mol of solid sodium fluoride is produced and 409.2kJ of heat is released. How much energy is released if one mole of sodium fluoride is produced? A gallon of water was heated from room temperature. 25 degree C, to almost boiling. 97 degree C. How much energy did the water absorb during this process? Given the thermochemical equation: 2Al(s) + 3/2 O_2(g) rightarrow Al_2O_3(s): delta H = -1, 676 kJ determine delta H for the following reaction: 2Al_2O_3(s) rightarrow 4Al(s) + 3O_2(g) Given the thermochemical reactions, calculate delta H for Na(s) + 1/2 Cl_2(g) rightarrow Na(g) + Cl(g): delta H = 230.0 kJ Na(s) + 1/2 Cl_2(g) rightarrow Nacl(s): delta H =-411 kJ Na(g) + Cl(g) rightarrow NaCI(s) Given the thermochemical reactions, calculate delta H of solid iron (III) bromide from the elements. Fe(s) + Br_2(l) rightarrow FeBr_2(s): delta H = -249.8 kJ FeBr_3 (s) rightarrow FeBr_2(s) + 1/2 Br_2(l): delta H = 18.4 kJ
Deanna HettingerLv2
3 Sep 2019