Use the equation that follows for parts (a) and (b) below. Molecular masses are under each salt/molecule. Al203 (s) + 6 NaOH (4 + 6 HF (g)→ 2 NasAIF6 (s) + 6 H2O (g) wwww 101.96 40.00 20.01 209.95 18.02 Part a) How many grams of aluminum oxide are needed to react with 3.5 L of HF at 305 K, 4.2 atm wwn pressure in the presence of excess NaOH? Part 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. Al203 (s) + 6 NaOH (4 + 6 HF (g)→ 2 NasAIF6 (s) + 6 H2O (g) wwww 101.96 40.00 20.01 209.95 18.02 Part a) How many grams of aluminum oxide are needed to react with 3.5 L of HF at 305 K, 4.2 atm wwn pressure in the presence of excess NaOH? Part b), How much energy is released from the reaction of 56.0 g of HF? Assume that H for the reaction is -345 kJ.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter6: The Gaseous State
Section: Chapter Questions
Problem 6.72QE: Nitrogen monoxide gas reacts with oxygen gas to produce nitrogen dioxide gas. What volume of...
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