Enthalpy - Page 2
Questions
- How can we convert #DeltaH_f^@# at 298K to #DeltaH_f^@# at different temperatures ?? Also tell how to convert bond energy at 298K to bond energy at different temperature
- Why are high heats of vaporization usually associated with high boiling temperature?
- The lattice energy of CsI(s) is −604 KJ/mol, and the enthalpy of solution is 33 KJ/mol. How would you calculate the enthalpy of hydration (KJ) of 0.65 moles of CsI? Enter a numeric answer only, do not include units in your answer?
- How many kilojoules are released when 111 g of #Cl_2# reacts with silicon in the reaction #Si(s)+2Cl_2(g) ->SiCl_4(g)# #ΔH = - 657kJ?#
- How can I calculate enthalpy of fusion?
- For the reaction #"N"_2(g) + "O"_2(g) -> 2"NO"(g) + "114.14 kJ"#, what mass of #"NO"# would need to be produced in order to release #"5.25 kJ"# of heat?
- How much energy is generated from freezing 2.5 g of water?
- How is #DeltaH_(fusion)# used to calculate the mass of solid that 1kJ of energy will melt?
- Why is enthalpy a state function?
- In an experiment at constant pressure, 4.24g of lithium chloride is dissolved in 100. mL of water at initial temperature of 16.3 degrees C. The final temperature of the solution is 25.1 degrees C. What is the enthalpy of solution in kJ/mol?
- How do you find delta h in a thermochemical equation?
- What is the standard enthalpy change of the formation of water?
- In the reaction #B_2H_6(g) + 3O_2(g) -> B_2O_3(s) + 3H_2O(g), ΔH = -2035 kJ#, how much heat is released when a mixture of #4.65# #g# #B_2H_6# and #2.94# #g# #O_2# is burned?
- Calculate the standard enthalpy change in kJ for the production of 12.2 g of H2O(l) from a reaction with the reactants: H2S(g), O2(g) and the products: H2O(l), SO2(g)?
- How much energy is needed to vaporize 5.00 g of water?
- What is an example of entropy? What is an example of enthalpy?
- What is the standard enthalpy of atomization?
- When 9.41 g of phenol, C6H5OH, are burned in a bomb calorimeter at 25 oC, 305.1 kJ of heat are given off. How to calculate the standard enthalpy of combustion, in kJ/mol, of phenol?
- How do you determine the enthalpy change for the reaction below using the enthalpy of combustion data in the table: #3C_((s)) +4H_(2(s)) -> C_3H_(8(s))#?
- What is the change in enthalpy for the final reaction?