Use the equation that follows for parts (a) and (b) below. Molecular masses are under each salt/molecule. Al2O3 (s) + 6 NaOH (l) + 6 HF (g) -> 2 Na3AlF6 (s) + 6 H2O (g) 101.96 40.00 20.01 209.95 18.02 a) How many grams of aluminum oxide are needed to react with 3.5 L of HF at 305 K, 4.2 atm pressure in the presence of excess NaOH? b) How much energy is released from the reaction of 56.0 g of HF? Assume that H for the reaction is -345 kJ.
Use the equation that follows for parts (a) and (b) below. Molecular masses are under each salt/molecule. Al2O3 (s) + 6 NaOH (l) + 6 HF (g) -> 2 Na3AlF6 (s) + 6 H2O (g) 101.96 40.00 20.01 209.95 18.02 a) How many grams of aluminum oxide are needed to react with 3.5 L of HF at 305 K, 4.2 atm pressure in the presence of excess NaOH? b) How much energy is released from the reaction of 56.0 g of HF? Assume that H for the reaction is -345 kJ.
Introductory Chemistry: A Foundation
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ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
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Use the equation that follows for parts (a) and (b) below. Molecular masses are under
each salt/molecule.
Al2O3 (s) + 6 NaOH (l) + 6 HF (g) -> 2 Na3AlF6 (s) + 6 H2O (g)
101.96 40.00 20.01 209.95 18.02
a) How many grams of aluminum oxide are needed to react with 3.5 L of HF at 305
K, 4.2 atm pressure in the presence of excess NaOH?
b) How much energy is released from the reaction of 56.0 g of HF? Assume that H
for the reaction is -345 kJ.
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