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1.) Determine the empirical and molecular formulas for a compound that has a molar mass of 62 g/mol and is 38.7% C 9.74% H and 51.6% O by mass.
2.) Suppose 11.89 g of iron is place in a stream of oxygen and completely reacts to give 16.99 g of the metal oxide, what would be the empirical formula for the metal oxide produce
3.) potassium chlorate decomposes to produce oxygen gas and potassium chloride. If you have 1.65 lbs of potassium chlorate how much oxygen (in grams) could be produced by the decomposition reaction? ___KClO->__KCl+___O
What is the electron configuration for Cuprous and Cupric, and since this is an exception to Aufbau, where are we removing electrons
Calculate the amount of work done against an atmospheric pressure of 1.00 atm when 500.0 g of zinc dissolves in excess acid at 30.0°C. Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)
Find ratio of the atomic mass of Silicon to Hydrogen if every 100g of SiH4 contains 87.45g of Si and 12.55g of H.
Calculate the ionic strength ad all the individual activity coeffcient for all solution in which 0.02 mole of (Feso4) and 0.1 mole of (NH4)2cro4
2C4H10 + 13O2 → 8CO2 + 10H2O The equation shows the combustion of butane (C4H10). How many moles of water can be produced by 12.5 moles of C4H10 with excess oxygen.
When aluminum crystalizes, it forms face-centered cubic cells. The atomic radius of an Al atom is 143. Caluculate the density of metallic aluminum.
Which one of the ions (i) Cl- and (ii) Ce3+ will be oxidized by MnO4- in acidic solution? Write balanced equations for these and calculate the standard potential for each reaction?
The partial pressure of oxygen gas in an atmosphere at STP is approximately 0.2 atm. If I capture 11.2 liters of atmospheric gas at STP in a flask,
Classify the set of solutions based on the movement of solvent from the first solution listed to the second solution listed as osmosis or reverse osmosis.
a student prepared a stock solution by dissolving 10.0g of koh in water to make 150. ml of solution. she then took 15.0
Calculate the molarity of a solution made by dissolving 0.140 mol Na2SO4 in enough water to form exactly 800mL of solution.
How many L of O2 gas at STP, are needed to react with 15.0 g of Na using the following chemical reaction: 2Na(s) + O2(g) => 2NaO(s)?
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