Reaction between 200 cm³ of 0.1M H₂SO₄ and a Metal
In this reaction, we will explore the interaction between 200 cm³ of 0.1M sulfuric acid (H₂SO₄) and a metal. Sulfuric acid is a strong acid that can react with metals to produce hydrogen gas and a salt.
The Reaction Equation
The reaction equation for this interaction can be written as:
Metal (M) + H₂SO₄ → M₂(SO₄)₃ + H₂
Calculating the Number of Moles of H₂SO₄
To calculate the number of moles of H₂SO₄, we need to know the volume (in liters) and the concentration (in moles per liter) of the acid. Since we have 200 cm³ of 0.1M H₂SO₄, we can convert the volume to liters as follows:
200 cm³ = 200/1000 L = 0.2 L
Now, we can calculate the number of moles of H₂SO₄:
Number of moles = Concentration x Volume = 0.1 mol/L x 0.2 L = 0.02 mol
The Metal's Role in the Reaction
The metal (M) reacts with the sulfuric acid to produce a salt and hydrogen gas. The type of metal used will affect the outcome of the reaction. For example, if we use zinc (Zn) as the metal, the reaction would be:
Zn + H₂SO₄ → Zn₂(SO₄)₃ + H₂
Factors Affecting the Reaction
Several factors can affect the reaction between the metal and the sulfuric acid. These include:
- Concentration of the acid: Increasing the concentration of the acid will increase the rate of reaction.
- Surface area of the metal: Increasing the surface area of the metal will also increase the rate of reaction.
- Temperature: Increasing the temperature will increase the rate of reaction.
Conclusion
In conclusion, the reaction between 200 cm³ of 0.1M H₂SO₄ and a metal is an important chemical reaction that can produce a salt and hydrogen gas. The type of metal used, the concentration of the acid, the surface area of the metal, and the temperature can all affect the outcome of the reaction.
