Answer to Question #301218 in Chemistry for Kyle

Question

1. At 733 mmHg and 114.8oF, calculate the density of HBr gas. Complete solution

Answer 1

The molar mass of HBr is 80.9 g mol⁻¹

R = gas constant = 0.0821 L atm K⁻¹ mol⁻¹

Converting units:

P = (733 mmHg) × (1 atm / 760 mmHg) = 0.9645 atm

T = (114.8^oF + 459.67) × (5/9) = 319.15 K

Solution:

The ideal gas equation can be used.

PV = nRT

Moles (n) = Mass (m) / Molar mass (M)

Therefore, the ideal gas equation can be rewritten as:

PV = (m/M)RT

PVM = mRT

Density (d) = Mass (m) / Volume (V)

Rearrange the equation to make d the subject:

d = m / V = PM / RT

d = PM / RT

Therefore,

Density of HBr gas = (0.9645 atm × 80.9 g mol⁻¹) / (0.0821 L atm K⁻¹ mol⁻¹ × 319.15 K) = 2.978 g/L

Density of HBr gas = 2.978 g/L = 2.98 g/L

Answer: The density of HBr gas is 2.98 g/L