In a chemical reaction you collect 1L Hydrogen gas at STP. How many moles of hydrogen gas did you collect?

This query provides us with:

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To find the number of moles of hydrogen gas collected at STP, we can use the ideal gas law equation, which states:

$PV = nRT$

Where:

• $P$ is the pressure of the gas (in atmospheres, atm)
• $V$ is the volume of the gas (in liters, L)
• $n$ is the number of moles of gas
• $R$ is the ideal gas constant (0.0821 L·atm/mol·K)
• $T$ is the temperature of the gas (in Kelvin, K)

At STP (Standard Temperature and Pressure), the pressure ($P$) is 1 atmosphere (atm) and the temperature ($T$) is 273.15 Kelvin (K).

Given that the volume ($V$) is 1 liter (L), the pressure ($P$) is 1 atmosphere (atm), and the temperature ($T$) is 273.15 Kelvin (K), we can rearrange the ideal gas law equation to solve for the number of moles ($n$):

$n = \frac{PV}{RT}$

Plugging in the values:

$n = \frac{(1 \, \text{atm})(1 \, \text{L})}{(0.0821 \, \text{L}·\text{atm/mol}·\text{K})(273.15 \, \text{K})}$

$n = \frac{1}{22.414}$

$n \approx 0.0446 \, \text{moles}$

Therefore, you collected approximately 0.0446 moles of hydrogen gas at STP.