Question

ammonia gas decomposes according to the equation:
$2\ce{nh3}(g) \
ightarrow \ce{n2}(g) + 3\ce{h2}(g)$

if 12.0 l of nitrogen is formed at stp, how many liters of hydrogen will be produced (also measured at stp)?

\\(\bigcirc\\) 12.0 l
\\(\bigcirc\\) 24.0 l
\\(\bigcirc\\) 36.0 l
\\(\bigcirc\\) not enough information

question 33 (0.0862 points)

which of the substances listed below is a nonpolar molecule?

\\(\bigcirc\\) \\(\ce{cl2o}\\)
\\(\bigcirc\\) \\(\ce{sicl4}\\)
\\(\bigcirc\\) \\(\ce{h2o2}\\)

Explanation:

First Question (Ammonia Decomposition)

Step1: Identify Mole Ratio

From the reaction \(2\text{NH}_3(\text{g})
ightarrow \text{N}_2(\text{g}) + 3\text{H}_2(\text{g})\), the mole ratio of \(\text{N}_2\) to \(\text{H}_2\) is \(1:3\). At STP, volume ratios equal mole ratios for gases.

Step2: Calculate Volume of \(\text{H}_2\)

Given volume of \(\text{N}_2 = 12.0\) L. Let volume of \(\text{H}_2\) be \(V\). Using the ratio \(\frac{V_{\text{H}_2}}{V_{\text{N}_2}}=\frac{3}{1}\), so \(V_{\text{H}_2}=3\times V_{\text{N}_2}=3\times12.0 = 36.0\) L.

• \(\text{Cl}_2\text{O}\): Bent structure, polar bonds (Cl - O) with net dipole moment (polar).
• \(\text{SiCl}_4\): Tetrahedral geometry, symmetric, polar bonds (Si - Cl) cancel out (nonpolar).
• \(\text{H}_2\text{O}_2\): Asymmetric structure, polar bonds with net dipole (polar).

Answer:

36.0 L (corresponding to the option "36.0 L")

Second Question (Nonpolar Molecule)