# Problem: For the following reaction, what is ∆H° when 25.0 g of Na2O2(molar mass = 77.98 g mol−1) is reacted with water?2 Na2O2(s) + 2 H2O(l) → 4 NaOH(s) + O2(g)         ∆H° = −126 kJ(A) -20.2 kJ (B) 87.4 kJ (C) -126 kJ (D) 20.2 kJ (E) -87.4 kJ

###### FREE Expert Solution

Use the concept of thermochemistry and stoichiometry to determine ΔH of the reaction of 25 g Na2O2 upon reaction with water

It can be seen that 2 moles of Na2O2 produces -126 kJ of heat.

Calculating for the ΔH of the reaction:

86% (488 ratings)
###### Problem Details

For the following reaction, what is ∆H° when 25.0 g of Na2O2(molar mass = 77.98 g mol−1) is reacted with water?

2 Na2O2(s) + 2 H2O(l) → 4 NaOH(s) + O2(g)         ∆H° = −126 kJ

(A) -20.2 kJ

(B) 87.4 kJ

(C) -126 kJ

(D) 20.2 kJ

(E) -87.4 kJ

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equations concept. You can view video lessons to learn Thermochemical Equations Or if you need more Thermochemical Equations practice, you can also practice Thermochemical Equations practice problems .

What is the difficulty of this problem?

Our tutors rated the difficulty of For the following reaction, what is ∆H° when 25.0 g of Na2O2... as low difficulty.