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Write a balanced chemical equation for the reaction between MnO4- and I - in basic solution. The skeleton ionic reaction is given below. MnO4-(aq) + I -(aq) MnO42-(aq) + IO3-(aq)
Calculate the power required to compress 10kg/s of air from 1atm and 57 degree C to 3atm and 707 degree C
aluminum oxide decomposes to produce aluminum metal and oxygen gas. when 9.8g of aluminum oxide decomposes how many
A mixture of ethanol and 1-proponol behaves ideally at 36 degrees celcius and is in equillibrium with its vapor. If the mole fraction of ethanol in the solution 0.49, calculate the mole fraction in the vapor phase at this temperature.
A mixture of neon and oxygen gases at a total pressure 975 mm Hg contains neon at a partial pressure of 325 mm Hg. If the gas mixture contains 3.75 grams of neon,
Use Hess' Law to show how the titration of acetic acid with sodium hydroxide can be expressed as the combination of two reactions: the acetic acid reacting with water, and the sodium hydroxide reacting with hydronium ion.
A 2-kg mass of an ideal gas expands at a constant pressure of 172 kPa in a piston-cylinder system from a temperature of 32oC to a final temperature of 182oC. Determine Q, W, DeltaU and DeltaH.
What mass (in grams) of solid KCl would need to be added to 500 grams of water to make an ideal solution with a boiling point of 106.8
The value that should be reported for the number of moles of gas calculated from the ideal gas equation given the following data (R = 0.08206 L•atm/mol•K, P = 76.00 cmHg, V = 1.000 L, and t = 1°C) is
Hex-1-ene, 2-methylpent-2-ene, 2,3-dimethylbut-2-ene, (Z)-hex-2-ene, (E)-hex-2-ene Which one has the highest boiling point and why
celcius of a solution prepared by dissolving 0.0550 mole of a sodium acetate in 1.00 L of 0.250 M acetic acid.
Complete combustion of 7.60 g of a hydrocarbon produced 24.3 g of CO2 and 8.70 g of H2O. What is the empirical formula for the hydrocarbon?
The empirical formula of a compound is found to be P2O5. Experiments show that the molar mass of the compound is 560g/mol. What is the molecular formula of the compound?
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