Question

Question 16
Balance the following the chemical equation:
____Ti3N+_____MgO---->_____Mg3N2+_____Ti2O

Answer 1

To balance the chemical equation \( \text{Ti}_3\text{N} + \text{MgO} \rightarrow \text{Mg}_3\text{N}_2 + \text{Ti}_2\text{O} \), we need to ensure that the number of each type of atom is the same on both sides of the equation.

Let's break it down step by step.

1. **Identify the number of atoms for each element on both sides:**
- Reactants:
- Titanium (Ti): 3 from Ti3N
- Nitrogen (N): 1 from Ti3N
- Magnesium (Mg): 1 from MgO
- Oxygen (O): 1 from MgO

- Products:
- Magnesium (Mg): 3 from Mg3N2
- Nitrogen (N): 2 from Mg3N2
- Titanium (Ti): 2 from Ti2O
- Oxygen (O): 1 from Ti2O

2. **Start balancing the elements.**
- To balance nitrogen:
- We have 1 nitrogen on the reactant side and 2 on the product side (in Mg3N2), so we need to have 2 Ti3N on the left:
- Update: \( 2\text{Ti}_3\text{N} + \text{MgO} \rightarrow \text{Mg}_3\text{N}_2 + 2\text{Ti}_2\text{O} \)

3. **Adjust for the number of magnesium and titanium:**
- After adjusting for nitrogen, we see we still have:
- Titanium: \( 2 \times 3 = 6 \) in \( 2\text{Ti}_3\text{N} \) and \( 2 \times 2 = 4 \) in \( 2\text{Ti}_2\text{O} \)
- Magnesium: 3 on the product side.

4. **Balance the magnesium:**
- We need 3 magnesium on the reactant side, so place a 3 in front of \( \text{MgO} \):
- Update: \( 2\text{Ti}_3\text{N} + 3\text{MgO} \rightarrow \text{Mg}_3\text{N}_2 + 2\text{Ti}_2\text{O} \)

5. **Count again:**
- Reactant side:
- Ti: 6 (from \( 2\text{Ti}_3\text{N} \)), N: 2 (from 2 Ti3N), Mg: 3 (from 3 MgO), O: 3 (from 3 MgO).
- Product side:
- Mg: 3 (from Mg3N2), N: 2 (from Mg3N2), Ti: 4 (from \( 2\text{Ti}_2\text{O} \)), O: 2 (from \( 2\text{Ti}_2\text{O} \)).

So the balanced equation is:

\[ 2\text{Ti}_3\text{N} + 3\text{MgO} \rightarrow \text{Mg}_3\text{N}_2 + 2\text{Ti}_2\text{O} \]

Final coefficients are:
\[
\boxed{2}\text{Ti}_3\text{N} + \boxed{3}\text{MgO} \rightarrow \boxed{1}\text{Mg}_3\text{N}_2 + \boxed{2}\text{Ti}_2\text{O}
\]

Answer 2

Question 17
Which of the following is NOT a way to speed up a chemical reaction? (Select all that apply)

a
decreasing the temperature of one of the reactants
b
decreasing the surface area of one of the reactants
c
increasing the concentration of one of the reactants
d
increasing the temperature of one of the reactants

Answer 3

To determine which options are NOT ways to speed up a chemical reaction, let's evaluate each one:

a) **Decreasing the temperature of one of the reactants**
This would slow down the reaction because lower temperatures generally lead to fewer collisions between reactant molecules.

b) **Decreasing the surface area of one of the reactants**
Reducing the surface area (for example, by using larger chunks instead of powders) would also slow down the reaction because fewer particles are available for collision.

c) **Increasing the concentration of one of the reactants**
Increasing concentration generally speeds up a reaction because it increases the likelihood of collisions between reactant molecules.

d) **Increasing the temperature of one of the reactants**
Increasing temperature usually speeds up a reaction because it elevates the kinetic energy of the molecules, resulting in more frequent and more energetic collisions.

Based on this analysis, the options that are NOT ways to speed up a chemical reaction are:

- **a (decreasing the temperature of one of the reactants)**
- **b (decreasing the surface area of one of the reactants)**

So the correct answers are **a** and **b**.