How many moles of gas are there in a 45.0 l container at 25.0 °c and 500.0 mm hg?

You can solve this by utilizing the ideal gas law, PV=nRT. P is pressure, V is volume, n is the number of moles, R is a constant (depends on the unit of pressure), and T is the temperature (in Kelvins).

500.0mmHg- convert to atm

=0.65789atm (do sig figs last)

25.0 C- convert to K

25.0 +273= 298K

PV=nRT

0.65789atm times 45.0L equals n (the variable) times R (0.08206L atm mol^-1 K^-1) times 298K

Isolate the variable, n and plug into a calculator.

I hope this helped!

The moles of gas is 1.21 moles.

Explanation:

To calculate the moles of gas, we use the equation given by ideal gas which follows:

where,

P = pressure of the gas = 500.0 mmHg  

V = Volume of the gas = 45.0 L

T = Temperature of the gas =

R = Gas constant =

n = number of moles of gas = ?

Putting values in above equation, we get:

Hence, the moles of gas is 1.21 moles.

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3