How many moles of gas occupy 56.3 L at 0.899 atm and 20.0°C?

n = 2.1 mol

Explanation:

Given data:

Number of moles of gas = ?

Volume of gas = 56.3 L

Pressure of gas = 0.899 atm

Temperature of gas = 20°C (20+273 = 293 k)

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

0.899 atm × 56.3 L  = n × 0.0821 atm.L/ mol.K  × 293 k

50.614 atm.L = n × 24.055 atm.L/ mol

n = 50.614 atm.L / 24.055 atm.L/ mol

n = 2.1 mol

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation:

false

because it does not have the potential to be entirely used up