Given

• V₁ = 750 cc (initial volume)
• T₁ = -3°C = 270 K (initial temperature in Kelvin)
• V₂ = 1 litre = 1000 cc (final volume)
• T₂ is the final temperature in Kelvin.

Using the formula:

750\over270 = 1000\over\text{T}_2

or, T₂ = (1000 × 270) \over 750

T₂ = 360 K

Converting T2 back to Celsius:

T₂ = 360 K – 273 = 87°C

So, the final temperature is 87°C.

OR

Given

• Pressure (P) = 4 atm
• Volume = V (what we need to find)
• number of moles = n
• R = 0.082 L·atm·mol⁻¹·K⁻¹
• Temperature (T) = 27°C + 273 = 300 K

Number of moles (n) = 8\over2 = 4 mol

PV = nRT

or, 4 × V = 4 × 0.082 × 300

or, V = 4 × 0.082 × 300\over 4 = 24.6 L

So, the volume of 8 g of H₂ gas is 24.6 liters.