Hydrogen gas H2 is the least dense of all gases. A sample of H2 gas is found to occupy a volume of 1.23 L at 755 mmHg and 0 ◦C. What volume , in liters, will this same gas occupy at .97 atm and a temperature of 50 ◦C.(10 points) Please include equation used, variable you solved for and answer with correct units

V₂ = 1.48 L

Explanation:

Given data:

Initial volume = 1.23 L

Initial pressure = 755 mmHg (755/760 =0.99 atm)

Initial temperature = 0 °C (0 +273 = 273 K)

Final temperature = 50°C (50+273 = 323 K)

Final volume =  ?

Final pressure = 0.97 atm

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 0.99 atm × 1.23 L × 323 K / 273 K × 0.97 atm

V₂ = 393.32 atm .L. K / 264.81 atm.K

V₂ = 1.48 L

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