Author: Anonymous

When 1 mol of potassium chlorate crystals, KClO3, decompose to potassium chloride crystals and oxygen gas at constant temperature and pressure, 39.0 kJ of heat is given off.  Write a thermochemical equation for this reaction. [Make sure to use subscripts and superscripts where applicable.  If you need any Greek symbols or arrows,  they are located in the math equation (square root symbol) in the tool bar immediately above this question.]

The decomposition of iodine pentafluoride be represented by the equation:     IF5(g)  →  IF3(g) + F2(g)  ΔH = ? Use the following information to find ΔH for the reaction above.     IF(g)  + F2(g) →  IF3(g)   ΔH = -390. kJ     IF(g)  + 2F2(g) →  IF5(g)   ΔH = -745 kJ                      

Use standard enthalpies of formation provided to calculate ΔHorxn for the following reaction: C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) Substance ΔHof (kJ/mol) C2H5OH(l) -277.6 CO2(g) -393.5 O2(g) 0 H2O(g) -241.8

What is the wavelength, in m, of a photon having a frequency of 87.9 ks-1?  (If you wish, you can show math work for possible partial credit.)

When 1 mol of potassium chlorate crystals, KClO3, decompose to potassium chloride crystals and oxygen gas at constant temperature and pressure, 39.0 kJ of heat is given off.  Write a thermochemical equation for this reaction. [Make sure to use subscripts and superscripts where applicable.  If you need any Greek symbols or arrows,  they are located in the math equation (square root symbol) in the tool bar immediately above this question.]

Match: Note there are more matching possibilities than needed.

  Equations:              q = (m)(c)(ΔT)              1 cal = 4.184 J                   ΔH°rx = ∑n  ΔHf°products − ∑n ΔHf°reactants E = hc/

Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of 5.49 × 1014 s-1.  

Which of the following combinations of quantum numbers is permissible?

Using the following equation for the combustion of octane, calculate the amount of heat involved when  0.7520 moles  of  octane react.   2 C8H18 + 25 O2  → 16 CO2 + 18 H2O                         ΔH°rxn = -11018 kJ (If you wish, you can show math work for possible partial credit.)