Question

modern vacuum techniques make it possible to reach a pressure of 1.00 * 10 ^ -10 mm Hg in a laboratory system. what volume in milliliters would 1.00 * 10 ^ 6 molecules of gas occupy at this pressure and standard temp?​

Answer 1

Answer:

The volume occupied by the 1.00 × 10⁶ moles of the gas at 1.00 × 10⁻¹⁰ mmHg and 273.15 K is 1.70 × 10²³ millilitres

Explanation:

Here we have the universal gas equation given by the equation;

PV = nRT

Therefore,

$V = \frac{nRT}{P}$

Where:

V = Volume occupied by the gas

n = Number of moles = 1.00 × 10⁶ moles

R = Universal gas constant = 62.363 mmHg·L/(mol·K)

T = Temperature = 273.15 K  (Standard Temperature)

P = Pressure = 1.00 × 10⁻¹⁰ mmHg

Plugging in the values, we have;

$V = \frac{1.00 \times 10^6 \times 62.363 \times 273.15}{1.00 \times 10^{-10} } = 1.703 \times 10^{20} \ liters$

Therefore the volume, V in millilitres = 1000 × 1.703 × 10²⁰ l

Volume,V in millilitres = 1.703 × 10²³ millilitres.