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Suppose that the microwave radiation has a wavelength of 12.4cm . How many photons are required to heat 275mL of coffee from 25.0 ?C to 62.0 ?C? Assume that the coffee has the same density, 0.997g/mL , and specific heat capacity, 4.184J/(g?K) , as water over this temperature range.
What is the molar concentration of the excess reactant once this reaction has finished? (40%)
Volume of added base required to reach the equivalence point? State the pH at one half of the equivalence point
Patients suffering from respiratory disorders are often treated in oxygen tents in which the atmosphere is enriched in oxygen. What is the partial pressure of O2 in an oxygen tent consisting of 45% O2 for an atmospheric pressure of 753 mm Hg?
The minerals chalcocite (Cu2S) and malachite (Cu2CO3(OH)2) are two primary sources of copper. What is the oxidation state of copper in each of these minerals?
If 18.08 grams of ammonia (NH3) react, how many grams of water should theoretically be produced?
At equilibrium the pressure of NH3 (g) is 1.23 atm. NH4Cl (s) ---> NH3 (g) + HCl (g) Find the equilibrium constant Ka for the reaction
Concentration of NADH was found by using beer's law using 6.22 mM cm-1 as extinction coefficient. Concentration of NADH = .0212 mM. Moles of NADH that are present in 1.02 mL sample was found by : .0212 mM x 1.02 mL = .021624 mM/mL
What volume of .250 M NaOH is required to neutralize a 10mL sample of .750 M HCl.
A gas has a pressure of 4.82035 atm when its volume is 2.75 L. What will the pressure be when the volume is changed to 1.91015 L, assuming constant temperature.
A 15.0--mL unknown sample of aqueous acetic acid, CH3COOH(aq), was titrated using 0.800 M NaOH. If the titration endpoint was found to be 20.0 mL.
A sample of water 53 g with a temperature of thirty six degree celsius is combined to 250 grams of H 2 O at 91 degree Celsius in an insulated container. Determine the final temperature after thermal equilibrium is reached?
When ethylamine, a weak base (Kb=4.3E-4), reacts with the formic acid, a weak acid (Ka=1.8E-4), the following reaction takes place: Calculate K for this reaction.
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