A 10.0 g piece of pure aluminum is placed in 75.0 mL of 0.54 M
hydrochloric...
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Chemistry
A 10.0 g piece of pure aluminum is placed in 75.0 mL of 0.54 Mhydrochloric acid at STP condition. They react as follows: 2Al +6HCl → 3H2(g) + 2AlCl3 Calculate the following:
a. Volume, in liters, of hydrogen gas.
b. Molarity of Al+3. (Assume 75.0 mL solution.)
c. Molarity of Cl–. (Assume 75.0 mL solution.)
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Answer We are given mass of Al 100 g Molarity of HCl 054 M volum e of HCl 750 mL Reaction 2Al 6HCl 3H2g 2AlCl3 Now first we need to calculate the moles of each reactant Moles of Al 100 g 26982 gmol1 0371 moles Moles of HCl 054 M 0075 L
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