You have a 5-liter container with 2.00 x 1023 molecules of ammonia gas (nh3) at stp
how many molecules of argon gas (ar) are in an identical container at the same temperature
and pressure?
6.02 x 1024 molecules
1.30 x 1024 molecules
2.00 x 1023 molecules
6.02 1023 molecules

1.34×10²³ molecules

Explanation:

Given data:

Volume of container = 5 L

Number of molecules of ammonia = 2.00×10²³

Number of molecules of Ar = ?

Volume of container = 5 L

Temperature = 273 K

Pressure = 1 atm

Solution:

PV = nRT

n = PV/RT

n = 1 atm. 5 L / 0.0821 atm. L. mol⁻¹. K⁻¹ . 273.15 K

n = 5 L.atm /22.426 atm. L. mol⁻¹.

n = 0.223 mol

Number of molecules of argon:

One mole = 6.02 ×10²³ molecules

0.223 mol

6.02 ×10²³×0.223

1.34×10²³ molecules

the ratio of the conjugate base to the acid required to attain the desired ph.

the formula for the conversion of temperature from degree celsius to kelvin is:

the sample of water at is converted to kelvin temperature by using the above formula as:

on comparing the two samples of water at or we can say that at and at respectively. the difference between the temperatures of two samples of water is:

hence, one can say that the sample of water at is greater than the sample of water at by .