How might the ideal gas law explain the atmospheric expansion during the Santa Ana winds? Decreased altitude reduces particle velocity. Amospheric gases condense at lower temperatures. Increased temperature causes gas particles to expand in volume Increased pressure creates colder air.

## Step 1<br />The ideal gas law is a fundamental principle in the study of gases. It states that the pressure exerted by a gas is directly proportional to its temperature and inversely proportional to its volume, assuming the amount of gas is constant. This relationship is mathematically represented as:<br />### \( PV = nRT \)<br />where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the gas constant, and \( T \) is the temperature.<br /><br />## Step 2<br />The Santa Ana winds are known for their high temperatures and low humidity. This means that the temperature of the air is high and the volume of the air is relatively constant.<br /><br />## Step 3<br />According to the ideal gas law, if the temperature increases while the volume remains constant, the pressure will also increase. However, in the case of the Santa Ana winds, the pressure is not increasing, but the volume is.<br /><br />## Step 4<br />Therefore, the ideal gas law explains the atmospheric expansion during the Santa Ana winds by stating that the increased temperature causes gas particles to expand in volume. This is because the volume of the air is relatively constant, and the temperature is increasing, so the volume must increase to accommodate the increased temperature.