Calculate the heat of reaction per mole of water if addition of 25.0 mL of 0.101 M A H2SO4 to 50.0 mL of 0.103 M NaOH causes the temperature to rise by 0.99°C. Assume that for both solutions the density is 1.00 g/mol and the specific heat (s) = 4.184 J/g °C. %3D
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
![**Calculating the Heat of Reaction per Mole of Water**
**Problem Statement:**
Calculate the heat of reaction per mole of water if the addition of 25.0 mL of 0.101 M H₂SO₄ to 50.0 mL of 0.103 M NaOH causes the temperature to rise by 0.99°C.
**Assumptions:**
- The density of both solutions is 1.00 g/mL.
- The specific heat capacity (s) for the solutions is 4.184 J/g°C.
**Approach:**
1. **Determine the total mass of the solutions:**
\[ \text{Mass of H₂SO₄ solution} = 25.0 \text{ mL} \times 1.00 \text{ g/mL} = 25.0 \text{ g} \]
\[ \text{Mass of NaOH solution} = 50.0 \text{ mL} \times 1.00 \text{ g/mL} = 50.0 \text{ g} \]
\[ \text{Total mass (m)} = 25.0 \text{ g} + 50.0 \text{ g} = 75.0 \text{ g} \]
2. **Calculate the heat absorbed/released using the formula:**
\[ q = m \times s \times \Delta T \]
\[ q = 75.0 \text{ g} \times 4.184 \text{ J/g°C} \times 0.99 \text{°C} \]
\[ q = 310.611 \text{ J} \]
3. **Determine the moles of water produced:**
\[ \text{Moles of H₂SO₄} = 25.0 \text{ mL} \times 0.101 \text{ M} = 0.002525 \text{ mol} \]
\[ \text{Moles of NaOH} = 50.0 \text{ mL} \times 0.103 \text{ M} = 0.00515 \text{ mol} \]
Since H₂SO₄ reacts with NaOH in a 1:2 molar ratio:
\[ \text{Moles of NaOH needed} = 2 \times \text{Moles of H₂SO](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4a6e4794-5644-431d-9e96-b37fbaf0b60a%2Fe4e4d1dd-1c79-44eb-9d54-1a6f84638b07%2Fiw4ax9r_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
