Question
How many Carbon - Hydrogen bonds are in each molecule of methane? ___4___ (10 pts)
If there's 1652 kJ of bond energy in methane, how much energy is there in one C -H bond? ____413___ 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 __1650______ kJ of energy are _____released_____ So the reaction is __exothrmic__. (released or absorbed?)
If there's 1652 kJ of bond energy in methane, how much energy is there in one C -H bond? ____413___ 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 __1650______ kJ of energy are _____released_____ So the reaction is __exothrmic__. (released or absorbed?)
Answers
GPT-4o mini
Let's break down each part of your questions and fill in the blanks.
1. How many Carbon - Hydrogen bonds are in each molecule of methane?
- The answer is **4**. (Each methane molecule, CH₄, has 4 C-H bonds.)
2. If there's 1652 kJ of bond energy in methane, how much energy is there in one C -H bond?
- To find the energy per bond, divide the total bond energy by the number of C-H bonds.
- Calculation: \( \frac{1652 \, \text{kJ}}{4} \) = **413** kJ.
3. If there’s more bond energy in the reactants than the products, that reaction is
- The answer is **exothermic**. (Exothermic reactions release energy.)
4. If there’s less bond energy in the reactants than the products, that reaction is
- The answer is **endothermic**. (Endothermic reactions absorb energy.)
Now, for the last part:
5. Given that there are about 800 kJ/mol of energy in the C=O bond in carbon dioxide and about 500 kJ/mol of energy in the O=O bond in oxygen gas:
**When carbon and oxygen react**:
- The total bond energy for the products (CO₂) largely contributes to the energy changes, but let's assume you are meant to consider the resulting bond formations. A typical combustion reaction or formation reaction would be represented as:
- C + O₂ → CO₂
- The bond energy released in the formation of the products (CO₂) can be calculated as the energy of the bonds formed within the products minus the energy of the bonds broken in the reactants.
**So the reaction is**:
- The energy released during this process is presented as **1650** kJ of energy, and since this energy is released during the reaction, the answer for "are _____released_____" would be **released**.
Thus the final completion would be:
- When carbon and oxygen react **1650** kJ of energy are **released**. So the reaction is **exothermic**.
Please review this and confirm if you need any additional details or corrections!
1. How many Carbon - Hydrogen bonds are in each molecule of methane?
- The answer is **4**. (Each methane molecule, CH₄, has 4 C-H bonds.)
2. If there's 1652 kJ of bond energy in methane, how much energy is there in one C -H bond?
- To find the energy per bond, divide the total bond energy by the number of C-H bonds.
- Calculation: \( \frac{1652 \, \text{kJ}}{4} \) = **413** kJ.
3. If there’s more bond energy in the reactants than the products, that reaction is
- The answer is **exothermic**. (Exothermic reactions release energy.)
4. If there’s less bond energy in the reactants than the products, that reaction is
- The answer is **endothermic**. (Endothermic reactions absorb energy.)
Now, for the last part:
5. Given that there are about 800 kJ/mol of energy in the C=O bond in carbon dioxide and about 500 kJ/mol of energy in the O=O bond in oxygen gas:
**When carbon and oxygen react**:
- The total bond energy for the products (CO₂) largely contributes to the energy changes, but let's assume you are meant to consider the resulting bond formations. A typical combustion reaction or formation reaction would be represented as:
- C + O₂ → CO₂
- The bond energy released in the formation of the products (CO₂) can be calculated as the energy of the bonds formed within the products minus the energy of the bonds broken in the reactants.
**So the reaction is**:
- The energy released during this process is presented as **1650** kJ of energy, and since this energy is released during the reaction, the answer for "are _____released_____" would be **released**.
Thus the final completion would be:
- When carbon and oxygen react **1650** kJ of energy are **released**. So the reaction is **exothermic**.
Please review this and confirm if you need any additional details or corrections!