Question

the partial pressure of carbon dioxide in the atmosphere is 0.239 mmhg. calculate the partial pressure in atm and torr. round each of your answers to 3 significant digits.

Explanation:

Step1: Convert mmHg to atm

We know that \( 1\ atm = 760\ mmHg \). So to convert \( 0.239\ mmHg \) to atm, we use the conversion factor \( \frac{1\ atm}{760\ mmHg} \).
The calculation is \( 0.239\ mmHg\times\frac{1\ atm}{760\ mmHg}=\frac{0.239}{760}\ atm \approx 3.14\times 10^{-4}\ atm \) (rounded to 3 significant digits).

Step2: Convert mmHg to torr

We know that \( 1\ mmHg = 1\ torr \). So \( 0.239\ mmHg = 0.239\ torr \) (since the conversion factor between mmHg and torr is 1:1).

Answer:

• atm: \( 3.14\times 10^{-4}\)
• torr: \( 0.239\)