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A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the Kf for Cu(CN)42- is 1.0 × 1025, how much copper ion remains at equilibrium
calculate the stoichiometric air-fuel ratio of a fuel blend containing 80 vol.% ethanol and 20 vol.% gasoline
What are the differences between sub-energy levels and orbitals? (My professor said they were different.)
A 100.0ml sample of 0.100M methylamine(CH3NH2, kb=3.7x10-4) is titrated with 0.250M HNO3. Calculate the pH after the addition of each of the following volumes of acid. a) 0.0 ml b) 20.0 ml c) 40.0 ml d)60.0 ml
Calculate the Ksp for Na2B4O5(OH)4 from this data. d. What is the free energy change for the dissolution of Na2B4O5(OH)4 at this temperature?
Draw one specific example each of a beta-diketo compound and one example of an alpha
An Ice cube tray holds 325 grams of water. If the water initially has a temperature of 25 C, how many kilojoules of heat must be removed to cool and freeze the water 0 C?
randk the following solutions in order of increasing pH of their 0.1M aqueous solutions - KNO3, K2SO3, K2S
Consider the voltaic cell below, which is symmetric except for the fact that [Cu2+] is 1.0 M on the left side and 0.01 M on the right. Which electrode is +, and what is Ecell?
What volume will nitrogen gas occupy if the pressure is increased to 894 torr at constant temperature?
classify the reactions below as synthesis, decomposition, single replacement(cationic or anionic) or double replacement
indicate whether the signs of H and S are expected to be positive, negative or about 0. For each, indicate whether the process is always spontaneous, never spontaneous, spontaneous at high temperature or spontaneous at low temperature.
Determine the numbers of electron pairs (both bonding pairs and lone pairs) on the iodine atom in the following.
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