Answer:
Volume = 1.043L
Step-by-step explanation:
First off, we have to calculate the number of particles H2 at that condition have.
We were given the following;
Volume (V) = 0.584L
Temperature = 19.6°C + 273 = 292.6 K (Converting to Kelvin Temperature)
Pressure = 2.10 atm
Using the ideal gas equation;
PV = nRT,
where R = gas constant = 0.0821 L atm K−1 mol−1
making n subject of formular;
n = PV / RT
n = (2.1 * 0.584) / (0.0821 * 292.6)
n = 1.2264 / 24.02246
n = 0.05098 moles
Avogadro’s number is defined as the number of elementary particles (molecules, atoms, compounds, etc.) per mole of a substance. It is equal to 6.022×1023 mol-1
Number of particles present in 0.05098 moles of H2 is given as;
1 mole = 6.022×1023
0.05098 = x
Upon cross multiplication, we have;
x = 0.05098 * 6.022×1023 = 0.307×1023 = 3.07×1022 particles.
equal number of moles would have the same number of particles. So we just have to find the volume when the number of moles of Ar is 0.05098.
We were given the following for Ar;
Volume (V) = ?
Temperature = 53.6°C + 273 = 326.6 K (Converting to Kelvin Temperature)
Pressure = 1.31 atm
Using the ideal gas equation;
PV = nRT,
where R = gas constant = 0.0821 L atm K−1 mol−1
making V subject of formular;
V = nRT / P
V = ( 0.05098 * 0.0821 * 326.6) / 1.31
V = 1.043L