A Mixture of H2 an NH3 has a total pressure of 1.02 atm at 273k in a 0.75l container. If H2 is present in a mole fraction of 0.21, how many moles of NH3 are present?

We can solve this problem using the ideal gas law and the mole fraction concept. Here are the steps:

### Step 1: Use the Ideal Gas Law to find the total moles of gas.
The ideal gas law equation is:

\[
PV = nRT
\]

Where:
- \( P \) is the total pressure (1.02 atm),
- \( V \) is the volume of the container (0.75 L),
- \( n \) is the total moles of gas,
- \( R \) is the ideal gas constant (\( 0.0821 \, \text{L·atm/(mol·K)} \)),
- \( T \) is the temperature in Kelvin (273 K).

We can rearrange this equation to solve for \( n \):

\[
n = \frac{PV}{RT}
\]

Substituting the values:

\[
n = \frac{(1.02) \times (0.75)}{(0.0821) \times (273)}
\]

Let’s calculate the value of \( n \).

A Mixture of H2 and NH3 has a total pressure of 1.02 atm at 273K in a 0.75L container. If H2 is present in a mole fraction of 0.21, how many moles of NH3 are present?

Learn how to calculate the number of moles of NH3 in a gas mixture of H2 and NH3 with a total pressure of 1.02 atm at 273K in a 0.75L container. Using the Ideal Gas Law and the concept of mole fraction, this detailed solution is perfect for high school students in Grades 10-12.

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