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For each reaction below, (a) identify the oxidation states of the atoms and (b) identify the oxidant, reductant, species oxidized, and species reduced. Also, think about this: How many electrons are transferred in each reaction?O2 + 4 Fe2+ + 4 H3O+ ----> 6 H2O + 4 Fe3+H2SO4 + ClO- --- -> S(s) + ClO4- + H2O
Hydrogen is collected over water at .975 atm and 28 degrees Celsius. What is the partial pressure of H2?
if a container of nitrogen, oxygen, carbon dioxide has a pressure of 2.00atm and the partial pressure of O2 is 312torr,
Calculate the amount of heat liberated (in kJ) from 347 g of mercury when it cools from 85.0°C to 15.0°C.
Assuming a 75% recovery of the volume from the first filtration, what volume of cation solution will be used in part B of the procedure? (Hint: you started with 100ml and added NaOH)
What mass of C4H6 in grams is consumed in the reaction below when 36.9 grams O2 (g) are also consumed?
A 486 mL sample of water was cooled from 50.0°C to 10.0°C. Assuming a specific heat of 4.184 J/K g and a density of 1.00 g/mL, find the amount of heat transferred from the water to the surroundings.
Luminol is a reagent used to detect blood at crime scenes. A technician prepares a stock solution by adding 6.0 g of luminol (molar mass=177 g/mol) to 50.0 mL of H2O.
10.9g of ice at 0.00 degrees C is mixed with 50.0g of water at 32.0 degrees C. What is the final temperature of the mixture? (heat of fusion=333J/g; specific heats: ice=2.09J/gK; water=4.184J/gK
Under certain conditions, the formation of ammonia from nitrogen and hydrogen has an 8.12% yield. Under such conditions, how many grams of NH3 will be actually produced.
A 14.5 gram sample of gas is found to have a volume of 2.8 liters at 275 K and 1.10 atm. What is the molar mass of this gas?
A student takes 148. g of BaCl2, and reacts it according to the following equation: 3BaCl2 + Al2(SO4)3 → 3BaSO4 + 2AlCl3 How many moles of AlCl3 are formed?
Compute the equilibrium partial pressures of Carbon dioxide and CO gases. If equilibrium constant Kp for this reaction =1.52,
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