What is the density of hydrogen at STP conditions?A. 0.1 g/LB. 0.2 g/LC. 0.09 g/LD. 2 g/L

To find the density of hydrogen at STP (Standard Temperature and Pressure) conditions, we can use the following formula:

\[
\text{Density} = \frac{\text{Mass}}{\text{Volume}}
\]

At STP, the molar volume of any ideal gas (including hydrogen) is 22.4 liters (L), and the molar mass of hydrogen (H₂) is 2 grams per mole (since each hydrogen atom has a mass of approximately 1 gram, and there are 2 atoms in H₂).

Thus, the density of hydrogen at STP can be calculated as:

\[
\text{Density} = \frac{\text{Molar mass of hydrogen}}{\text{Molar volume at STP}} = \frac{2 \, \text{g}}{22.4 \, \text{L}}
\]

Now, let's compute this:

\[
\text{Density} = 0.0893 \, \text{g/L}
\]

Rounding this to two decimal places, we get approximately:

\[
\text{Density} \approx 0.09 \, \text{g/L}
\]

Thus, the correct answer is **C. 0.09 g/L**.