**Question 3:**How much heat in kilojoules is evolved in the reaction of 1.00 g of Na with H₂O?\[ \text{2Na(s) + 2H}_2\text{O(l) → 2NaOH(aq) + H}_2\text{(g)} \]\[ \Delta H° = -368.4 \, \text{kJ} \][Space for calculation or answer]**Explanation:**This question involves calculating the heat evolved during a chemical reaction between sodium (Na) and water (H₂O). The chemical equation provided shows the reaction producing sodium hydroxide (\[\text{NaOH}\]) and hydrogen gas (\[\text{H}_2\]). The enthalpy change (\[\Delta H°\]) is given as -368.4 kJ, indicating that the reaction is exothermic.**Graphs/Diagrams Explanation:**There are no graphs or diagrams included in this image.

Given :- 2Na(s) + 2H2O(l) ----> 2NaOH(aq) +H2(g) Delta Ho = -368.4 kJ To calculate :- Heat…

Answered: How much heat in kilojoules is evolved…

How much heat in kilojoules is evolved in the reaction of 1.00g of Na with H2O? 2Na(s) + 2H20(1) → 2NaOH(aq) + H2(g) AH° = -368.4kJ

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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