Question
How many Carbon - Hydrogen bonds are in each molecule of methane? ______ (10 pts)
If there's kJ of bond energy in methane, how much energy is there in one C -H bond? _______ kJ (10 pts)
If there’s more bond energy in the reactants than the products, that reaction is _exothermic__.(10 pts)
If there’s less bond energy in the reactants than the products, that reaction is
__endothermic_(10 pts)
There are about 800 kJ/ mol of energy in the C=O bond in carbon dioxide There are about 500 kJ/ mol of energy in the O=O bond in oxygen gas. Carbon alone has no bonds (so no bond energy).
When carbon and oxygen react ________ kJ of energy are __________ So the reaction is ____. (released or absorbed?)
If there's kJ of bond energy in methane, how much energy is there in one C -H bond? _______ kJ (10 pts)
If there’s more bond energy in the reactants than the products, that reaction is _exothermic__.(10 pts)
If there’s less bond energy in the reactants than the products, that reaction is
__endothermic_(10 pts)
There are about 800 kJ/ mol of energy in the C=O bond in carbon dioxide There are about 500 kJ/ mol of energy in the O=O bond in oxygen gas. Carbon alone has no bonds (so no bond energy).
When carbon and oxygen react ________ kJ of energy are __________ So the reaction is ____. (released or absorbed?)
Answers
GPT-4o mini
1. How many Carbon - Hydrogen bonds are in each molecule of methane? **4**
2. If there's \( kJ \) of bond energy in methane, how much energy is there in one C-H bond? **\( \frac{kJ}{4} \)** kJ (since there are 4 C-H bonds in methane).
3. If there’s more bond energy in the reactants than the products, that reaction is **exothermic**.
4. If there’s less bond energy in the reactants than the products, that reaction is **endothermic**.
5. There are about 800 kJ/mol of energy in the C=O bond in carbon dioxide, and there are about 500 kJ/mol of energy in the O=O bond in oxygen gas. The reaction you are referring to would be the combustion of carbon (like combustion of carbon to form carbon dioxide, for instance), so here's how energy is calculated:
- Total bond energy needed to break the bonds in the reactants:
- Break 1 O=O bond and 2 C=O bonds:
- 1 O=O bond = 500 kJ/mol
- 2 C=O bonds = 2 x 800 kJ/mol = 1600 kJ/mol
- Total = 500 + 1600 = 2100 kJ/mol
Assuming that carbon is being burned to form carbon dioxide:
- In combustion, C is combined with O2 to produce CO2, so the bond energy of reactants (O2 and C) is less than the bond energy of the products (CO2).
When carbon and oxygen react, **2100 kJ** of energy are **released**. So the reaction is **exothermic**.
2. If there's \( kJ \) of bond energy in methane, how much energy is there in one C-H bond? **\( \frac{kJ}{4} \)** kJ (since there are 4 C-H bonds in methane).
3. If there’s more bond energy in the reactants than the products, that reaction is **exothermic**.
4. If there’s less bond energy in the reactants than the products, that reaction is **endothermic**.
5. There are about 800 kJ/mol of energy in the C=O bond in carbon dioxide, and there are about 500 kJ/mol of energy in the O=O bond in oxygen gas. The reaction you are referring to would be the combustion of carbon (like combustion of carbon to form carbon dioxide, for instance), so here's how energy is calculated:
- Total bond energy needed to break the bonds in the reactants:
- Break 1 O=O bond and 2 C=O bonds:
- 1 O=O bond = 500 kJ/mol
- 2 C=O bonds = 2 x 800 kJ/mol = 1600 kJ/mol
- Total = 500 + 1600 = 2100 kJ/mol
Assuming that carbon is being burned to form carbon dioxide:
- In combustion, C is combined with O2 to produce CO2, so the bond energy of reactants (O2 and C) is less than the bond energy of the products (CO2).
When carbon and oxygen react, **2100 kJ** of energy are **released**. So the reaction is **exothermic**.