45.5 L of dinitrogen reacted with 22.7 L of dioxygen and 45.5 L of nitrous oxide was formed. The reaction is given below,`2N_2(g)+O_2(g) rarr 2N_2O(g)` Which law is being obeyed in this experiment ?

Options

A. Law of definite proportion
B. Law of conservation of mass
C. Law of multiple proportion
D. None of the above

Answer

To determine which law is being obeyed in the reaction of dinitrogen and dioxygen to form nitrous oxide, we can analyze the volumes of gases involved in the reaction step by step.

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction is:
\[ 2N_2(g) + O_2(g) \rightarrow 2N_2O(g) \]

### Step 2: Identify the volumes of the gases
From the problem statement:
- Volume of dinitrogen (\(N_2\)) = 45.5 L
- Volume of dioxygen (\(O_2\)) = 22.7 L
- Volume of nitrous oxide (\(N_2O\)) produced = 45.5 L

### Step 3: Analyze the volume ratios
According to the balanced equation:
- 2 volumes of \(N_2\) react with 1 volume of \(O_2\) to produce 2 volumes of \(N_2O\).

Now, let's check the volume ratios:
- For \(N_2\): 45.5 L corresponds to 2 volumes, so 1 volume would be \( \frac{45.5}{2} = 22.75 \) L.
- For \(O_2\): 22.7 L corresponds to 1 volume.
- For \(N_2O\): 45.5 L corresponds to 2 volumes.

### Step 4: Compare the ratios
From the reaction:
- The ratio of \(N_2\) to \(O_2\) is \(2:1\) (which is satisfied since \(22.75:22.7 \approx 2:1\)).
- The ratio of \(N_2\) to \(N_2O\) is also \(2:2\) or \(1:1\) (which is satisfied since \(45.5:45.5 = 1:1\)).

### Step 5: Conclusion
The volumes of gases react and produce in simple whole number ratios, which is a statement of **Gay-Lussac's Law of Combining Volumes**. This law states that when gases react together at constant temperature and pressure, they do so in volumes that are in the ratio of small whole numbers.

### Final Answer
The law being obeyed in this experiment is **Gay-Lussac's Law of Combining Volumes**.