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Aluminum bromide can be prepared by the reaction of aluminum metal with bromine gas shown by the equation:
2 Al + 3 Br2 --> 2 AlBr3
Now suppose that 5.6 g of aluminum reacts with 4.4 g of bromine. Calculate the following:
Calculate the mass of aluminum bromide that can be produced from 5.6 g of AL.
Calculate the mass of aluminum bromide that can be produced from 4.4 g of bromine.
Calculate the percent yield if the actual yield was 3.4 g AlBr3
Calculate the pH of a solution prepared by mixing 0.0800 mol of chloroacetic acid plus 0.0400 mol of sodium chloroacetate in 1.04 L of water. (pKa of chloroacetic acid = 2.865.)
write a report about the chemical equation about the combusiton of butane. the report must include the equation, a brief history about the combustion of butane and its importance to the world and any dangers involved.
When the liberated hydrogen gas is collected over water at 29 degrees celsius and 752 torr, the volume is found to be 343 mL. The vapor pressure of water at 29 degrees celsius is 30.0 torr. What is the mass percentage of aluminum in this alloy?
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