A sample of air in a syringe exerts a pressure of 1.03 atm at a temperature of 26.0^circ C The syringe is placed in a boiling water bath at 100.0^circ C. The pressure of the air is increased to 1.25 atm by pushing the plunger in, which reduces the volume to 0.233 mL. What was the original volume of air? "Round answer to thousandth place. That's 3 places after the decimal point. Type your answer.

## Step 1: We are given the initial pressure (P1), initial temperature (T1), final pressure (P2), and final temperature (T2). We need to find the initial volume (V1). We can use the ideal gas law, which states that the pressure of a gas times its volume is directly proportional to the temperature of the gas. This can be written as .## Step 2: First, we need to convert the temperatures from Celsius to Kelvin by adding 273.15. So, and .## Step 3: Next, we substitute the given values into the equation. We know that , , , , and . We need to solve for .## Step 4: Rearranging the equation to solve for , we get .## Step 5: Substituting the known values into the equation, we get \(V1 = (1.25 atm * 0.233 mL * 299.15 K) / (1.03 atm * 373.15 K)\).## Step 6: Calculating the above expression gives us the original volume of air.