Question

The ionization energy for potassium is 419 kJ/mol. The electron affinity for bromine is -325 kJ/mol....

The ionization energy for potassium is 419 kJ/mol. The electron affinity for bromine is -325 kJ/mol. Use these values and Hess's law to calculate the change in enthalpy for the following reaction per mole of reagent:

K(g)+Br(g)→K+(g)+Br−(g),      ΔH=?

Express your answer with the appropriate units.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The ionization energy for potassium is 419 kJ/mol. The wavelength of light emitted when an excited...
The ionization energy for potassium is 419 kJ/mol. The wavelength of light emitted when an excited K-atom undergoes the 4s ← 4p transition is approximately 769 nm. Using this information, calculate the energies of the 4s and 4p orbitals in potassium.​
Calculate the second ionization energy of the metal M (ΔHion2° in kJ/mol) using the following data:...
Calculate the second ionization energy of the metal M (ΔHion2° in kJ/mol) using the following data: Lattice enthalpy of MO(s), ΔHl° = -2297 kJ/mol Bond dissociation enthalpy of O2(g) = +498 kJ/mol First electron affinity of O = -141 kJ/mol Second electron affinity of O = +744 kJ/mol Enthalpy of sublimation of M = + 102 kJ/mol First ionization energy of M = + 340 kJ/mol Standard enthalpy of formation of MO(s), ΔHf° = -336 kJ/mol Refer to the textbook...
Given the following information: Energy of sublimation of K(s) = 77 kJ/mol Bond energy of HCl...
Given the following information: Energy of sublimation of K(s) = 77 kJ/mol Bond energy of HCl = 427 kJ/mol Ionization energy of K(g) = 419 kJ/mol Electron affinity of Cl(g) = –349 kJ/mol Lattice energy of KCl(s) = –705 kJ/mol Bond energy of H2 = 432 kJ/mol Calculate the net change in energy for the following reaction: 2K(s) + 2HCl(g) → 2KCl(s) + H2(g) ΔE = ______ kJ
Using the thermochemical data and an estimated value of -2235.2 kJ/mol for the lattice energy for...
Using the thermochemical data and an estimated value of -2235.2 kJ/mol for the lattice energy for potassium oxide, calculate the value for the second electron affinity of oxygen [O− + e- → O2−]. (The answer is 748.5 kJ/mol) Quantity Numerical Value (kJ/mol) Enthalpy of atomization of K 89 Ionization energy of K 418.8 Enthalpy of formation of solid K2O -363 Enthalpy of formation of O(g) from O2(g) 249.1 First electron attachment enthalpy of O   -141.0
Use Coulomb's law to calculate the ionization energy in kJ/mol of an atom composed of a...
Use Coulomb's law to calculate the ionization energy in kJ/mol of an atom composed of a proton and an electron separated by 114.00 pm . Express your answer ro\\to three significant figures with the appropriate units. part 2: What wavelength of light has sufficient energy to ionize the atom?
Calculate the lattice energy for NaF (s) given the following sublimation of energy +109 kj/mol Hf...
Calculate the lattice energy for NaF (s) given the following sublimation of energy +109 kj/mol Hf for F (g) + 77 kj/mol first ionization energy of Na (g) +495 electron affinity of F(g) -328 enthalpy of formation of NaF(s) -570 kj/mol A. -177 B. 192 C. -804 D. -1047 E. -923
te the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kJ/mol ∆Hf...
te the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kJ/mol ∆Hf for F(g) +77 kJ/mol first ionization energy of Li(g) +520. kJ/mol electron affinity of F(g) –328 kJ/mol enthalpy of formation of LiF(s) –617 kJ/mol A. none of these B. –650. kJ/mol C. 285 kJ/mol D. 800. kJ/mol E. 1052 kJ/mol
a)What is the ionization energy (in kJ/mol) for the one-electron species, He+1 ? b)What is the...
a)What is the ionization energy (in kJ/mol) for the one-electron species, He+1 ? b)What is the ionization energy (in kJ/mol) for the one-electron species, P+14 ?
Part A: The decomposition of NI3 to form N2 and I2 releases −290.0 kJ of energy....
Part A: The decomposition of NI3 to form N2 and I2 releases −290.0 kJ of energy. The reaction can be represented as 2NI3(s)→N2(g)+3I2(g), ΔHrxn=−290.0 kJ Find the change in enthaply when 15.0 g of NI3 decomposes. Express your answer to three significant figures and include the appropriate units. Part B: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure...
Given the following information: Li(s) → Li(g) enthalpy of sublimation of Li(s) = 166 kJ/mol HF(g)...
Given the following information: Li(s) → Li(g) enthalpy of sublimation of Li(s) = 166 kJ/mol HF(g) → H(g) + F(g) bond energy of HF = 565 kJ/mol Li(g) → Li+(g) + e– ionization energy of Li(g) = 520. kJ/mol F(g) + e– → F–(g) electron affinity of F(g) = -328 kJ/mol Li+(g) + F–(g) → LiF(s) lattice energy of LiF(s) = -1047 kJ/mol H2(g) → 2H(g) bond energy of H2 = 432 kJ/mol Calculate the change in enthalpy for: 2Li(s)...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT