Answer to Question #108611 in General Chemistry for Jonathan

Question

if 327.18 g C8H18 are burned what volume of O2 is needed if the pressure is 663.48 torr and the temperature is 70°C

Answer 1

Answer: 1,158 m³

Explanation:

Reaction: 2С₈Н₁₈ + 25О₂ → 16СО₂ + 18Н₂О

ν_С8Н18 =m/M = 327,18 g / 114 g/mol = 2,87 mol

Let's find v_O2 by proportion:

2 - 2,87

25 - v_O2

Herefrom,

v_O2= 2,87 • 25 / 2 = 35,875 mol

Next, let's use Ideal gas law pV = vRT

p = 664,48 torr = 88392,486 Pa

T = 70°C = 343,15 K

pV = vRT, herefrom

V_O2 = vRT/p = 35,875 mol • 8,314 J/mol•K • 343,15 K / 88392,486 Pa = 1,158 J/Pa = [Pa = J/m³] = 1,158 m³ or 1158 liters

Hopeful, my answer is comprehensive. Have a nice day and be healthy! :)