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Problem- Estimate the total work that can be obtained by combusting butane (C4H10) at 2700K. (assume liquid water is produced). State other assumptions.
Show all work, use additional paper if necessary.
Describe the bonding in SeO2 in valence bond terms. Note whether or not there is delocalized bonding and explain how molecular orbital theory can be useful here.
What is the solubility of M(OH)2 in pure water. B. What is the solubility of M(OH)2 in a .202 M solution of M(NO3)2? Ksp=5.45E-18
A bioengineer preparing cells for a cloning experiment bathes a small piece of rat epithelial tissue in a TRIS buffer, (HOCH2)3CNH2. The buffer is made by dissolving 34.0 g TRIS (pKb = 5.91) in enough 0.075 M HCl to make 1.00 L of solution.
During a strenuous workout an athlete generates 2050.0 kJ of heat energy. What mass of water would have to evaporate from the athletes skin to dissipate this much heat
Write a balanced overall equation for each isomer of stilbene (cis and trans)
How many grams of hydrogen would have to react to produce 71.9 kJ of energy from the reaction 2H2 + O2 --------> 2H2O + 484kJ?
How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18J(g*C). can someone explain this in detail. other descriptions don't answer this well and im lost when i try and do it
Calculate the number of moles of Ascobic acid in the 50.00 ml Sample. Titration Volumes of KIO3 Initial Buret reading/ml trial 1=12.54 trial 2=8.78 Final buret reading/ trial 1=38.74 trial 2=34.93 Volume of KIO used/ml trial 1=? trial 2=?
The element gallium has two naturally occurring isotopes with masses of 68.9300 amu and 70.9200 amu. What would be the fractional abundance of the first isotope, if the atomic weight was 69.6518 amu
lithium iodide has a lattice energy of -730 kjmol and a heat ofhydration of -793 kjmol. determine how much heat is
what mass of this substance must evaporate in order to freeze 180g of water initially. heat of fusion water is 334J/g; the specific heat of water is 4.18 J/g-k.
The PH of a solution prepared by dissolving 0.30 mole of the weak acid, HA, in enough water to make 1 liter of solution is 6.1. Calculate the Ka and the percent ionization of the HA solution.
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