What mass of aluminum chloride could theoretically be made from 8.1 g of aluminum and excess chlorine?

Answer 1

Approx. #40*g#

#"Moles of aluminum "=(8.1*g)/(26.98*g*mol^-1)# #=# #0.300*mol#

#Al(s) + 3/2Cl_2(g) rarr AlCl_3(s)#

Given the 1:1 stoichiometry between Al and the product, if all the aluminum were oxidized, #0.300*molxx133.34*g*mol^-1" aluminum trichloride"# would result, approx. 40 g.

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Answer 2

Peyton Adams

The molar mass of aluminum chloride is 133.34 g/mol. Aluminum has a molar mass of 26.98 g/mol. To find the theoretical yield of aluminum chloride, you need to determine the molar ratio between aluminum and aluminum chloride, which is 2:2. Therefore, the molar amount of aluminum chloride produced is the same as the molar amount of aluminum. Using the given mass of aluminum, you can calculate the theoretical yield of aluminum chloride.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.