Aqueous solution of aluminum bromide
How many mL of a 0.136 M aqueous solution of aluminum bromide, AlBr3, must be taken to obtain 17.3 grams of the salt?
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An unknown compound has the formula CxHyOz. You burn 0.220 g of the compound and isolate 0.312 g of CO2 and 0.191 g of H2O. What is the empirical formula of the compound? If the molar mass is 62.01 g/mol, what is the molecular formula?
How long would it take for 1.50mol of water at 100.0 degrees to be converted completely into steam if heat were added at a constant rate of 16.0J/s ? the constants are: Specific heat of ice: 2.09J(g/degrees celcius)
Find the gram formula mass of each compound.
The density of benzene at 15 degrees C is 0.8787 g/mL. Calculate the mass of 0.1500 L of benzene at this temperature.
What is the molarity of Cl^- ions in a solution formed by dissolving 7.20 g of the mixture in enough water to form 500.0 mL of solution?
Hydrogen and oxygen gas combine explosively to produce water. Write a balanced chemical equation for this process. If 10 mol of hydrogen reacted with oxygen, what volume of liquid water could be produced?
A volume of 95.0ml of h2o is initially at room temperature 22.0 C. A chilled steel rod at 2.00 *C.is placed in the water. If the final temperature of the system is 21.2 *C. What is the mass of the steel bar?
Molecular Mass by Freezing point Depression (Preliminary Lab) The following errors occurred when the above experiment was carried out. How would each affect the calculated molecular mass of the solute (too high,too low, no effect)? Explain your an
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