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A 2.50 l sample of nitrogen gas at 760 torr and 0.0 c weighs 2.60 g . The pressure on the gas is increased to 2.00 atm at 0.0 c . Calculate the density at the new pressure in g/l.
Accepted Answer
Here's how to calculate the density at the new pressure:
1. Convert the initial pressure to atmospheres:
760 torr = 1 atm
2. Apply Boyle's Law:
Boyle's Law states that the pressure and volume of a gas are inversely proportional at constant temperature. Mathematically, this is represented as P₁V₁ = P₂V₂.
We know:
P₁ = 1 atm
V₁ = 2.50 L
P₂ = 2.00 atm
We need to find V₂.
Solving for V₂:
V₂ = (P₁V₁) / P₂ = (1 atm
2.50 L) / 2.00 atm = 1.25 L
3. Calculate the density:
Density (ρ) is mass (m) divided by volume (V): ρ = m/V
m = 2.60 g
V = 1.25 L
ρ = 2.60 g / 1.25 L = 2.08 g/L
Therefore, the density of the nitrogen gas at the new pressure is 2.08 g/L.
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