**Chemical Reaction and Calculations**Use the equation that follows for parts (a) and (b) below. Molecular masses are under each salt/molecule.\[ \text{Al}_2\text{O}_3 (s) + 6 \, \text{NaOH} (l) + 6 \, \text{HF} (g) \rightarrow 2 \, \text{Na}_3\text{AlF}_6 (s) + 6 \, \text{H}_2\text{O} (g) \]Molecular masses:- $\text{Al}_2\text{O}_3$: 101.96- $\text{NaOH}$: 40.00- $\text{HF}$: 20.01- $\text{Na}_3\text{AlF}_6$: 209.95- $\text{H}_2\text{O}$: 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 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 $\Delta H$ for the reaction is -345 kJ.*

Answered: Use the equation that follows for parts…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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**Chemical Reaction and Calculations**

Use the equation that follows for parts (a) and (b) below. Molecular masses are under each salt/molecule.

\[ \text{Al}_2\text{O}_3 (s) + 6 \, \text{NaOH} (l) + 6 \, \text{HF} (g) \rightarrow 2 \, \text{Na}_3\text{AlF}_6 (s) + 6 \, \text{H}_2\text{O} (g) \]

Molecular masses:
- $\text{Al}_2\text{O}_3$: 101.96
- $\text{NaOH}$: 40.00
- $\text{HF}$: 20.01
- $\text{Na}_3\text{AlF}_6$: 209.95
- $\text{H}_2\text{O}$: 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 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 $\Delta H$ for the reaction is -345 kJ.*

Expert Solution

Step 1

The ideal law is sometimes considered as the combination of Boyle’s law, Charles’s law and Avogadro’s law. In general, this law relates the quantities like pressure, volume, amount of substance (number of moles) and temperature together. The expression of the ideal gas law is given below:

$P V = n RT$

Given data:

Volume of HF is 3.5 L

Temperature is 305 K

Pressure is 4.2 atm

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