Studdy AI Logo
Math

QuestionWhen 1 mol of NO(g)\mathrm{NO}(\mathrm{g}) forms from its elements, 90.29 kJ of heat is absorbed.
Part: 0 / 2
Part 1 of 2 Write a balanced thermochemical equation. (Include phases in your equation.) □\square

Studdy Solution

STEP 1

Assumptions
1. We are forming 1 mol of NO(g) from its elements.
2. The elements involved are nitrogen (N) and oxygen (O).
3. The reaction absorbs 90.29 kJ of heat, indicating it is endothermic.
4. The standard state of nitrogen is N₂(g) and oxygen is O₂(g).

STEP 2

Write the unbalanced chemical equation for the formation of NO(g) from its elements.
N2(g)+O2(g)→NO(g) \mathrm{N}_2(\mathrm{g}) + \mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{NO}(\mathrm{g})

STEP 3

Balance the chemical equation. Since NO contains one nitrogen and one oxygen atom, we need to ensure that the number of atoms of each element is the same on both sides of the equation.
12N2(g)+12O2(g)→NO(g) \frac{1}{2} \mathrm{N}_2(\mathrm{g}) + \frac{1}{2} \mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{NO}(\mathrm{g})

STEP 4

Include the thermochemical information in the balanced equation. Since the reaction absorbs 90.29 kJ of heat, we will add this information to the equation as a reactant.
12N2(g)+12O2(g)+90.29 kJ→NO(g) \frac{1}{2} \mathrm{N}_2(\mathrm{g}) + \frac{1}{2} \mathrm{O}_2(\mathrm{g}) + 90.29 \, \text{kJ} \rightarrow \mathrm{NO}(\mathrm{g})
The balanced thermochemical equation is:
12N2(g)+12O2(g)+90.29 kJ→NO(g) \frac{1}{2} \mathrm{N}_2(\mathrm{g}) + \frac{1}{2} \mathrm{O}_2(\mathrm{g}) + 90.29 \, \text{kJ} \rightarrow \mathrm{NO}(\mathrm{g})

Was this helpful?

Studdy solves anything!

banner

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

ParentsInfluencer programContactPolicyTerms
TwitterInstagramFacebookTikTokDiscord