This solution will discuss how to determine the enthalpy of a chemical reaction primarily using Hess's law. The use of the general formula for enthalpy will also be addressed. These problems will be solved using both Hess's law and the general formula for enthalpy. A step by step example and answers are included.
Detailed work would be very helpful; the math involved in this gets me confused, but I'm not sure where I have been going wrong. If work is handwritten, please do not write in cursive for I have problems reading it. 1. The mass of a substance is 200gm and its specific heat is 0.09. How much heat is required to raise the tempe
1. 2CLF (g) + O2(g) --> CL2O + F20 (Hrxn = 167.4 kj/mol) 2CLF3(g) + 2O2(g) --> Cl2O(g) + 3F2O(g) (Hrxn = 341.4 kj/mol) 2F2(g) + O2(g) --> 2F2O (Hrxn = -43.4 kJ/mol) Using Hess' law, what is the Hrxn for ClF +F2 --> ClF3 in kj/mol (assume temperature is the same)? 2. Given NO(g) + NO2(g) --> N2O3 H=-40.2kJ N2
1.) Calculate delta H for the following reaction: The reduction of aluminum oxide by hydrogen gas: Al2O3(s) + 3H2(g) ------- 2Al(s) + 3H2O(g) 2.) Solve for entalapy using Hess's Law. The standard heat of combustion of liquid ethyl alcohol is -227 kcal/mol and that of acetic acid is -209 kcal/mol. The equations are: C2
I am having trouble with a question in my homework. It states: Given the following thermochemical equations 2KCl(s) + 3O2(g) .......2KClO3(s) Change in H = 78.0kJ P4(s) + 6Cl2(g)..........4PCl3(g) Change in H = -1148.0kJ P4(s) + 2O2(g) + 6Cl2(g).........4POCl3(g)
See attached and directions.
Please answer step-by-step with solutions: A 150.0 iron bar at 330 degrees C is put in 1.00 kg water at 20.0 degrees C. What is the final temperature of the bar? (Hint: bar and water will be the same at the end.) Cs = 0.45J/(grams degree C) for iron Cs = 4.18J/(grams degree C) for water