both answers 5 Question 2) Considering the Ideal gas law; a) What is the Volume

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both answers 5

Question 2) Considering the Ideal gas law; a) What is the Volume (in Liter) of 5 mol of oxygen gas at 3.0 atm and at 50 °C? R= 0.0821 (L·atm/mol"K) b) What would be the Volume of 10 moles of gas at the same condition as the above question? Question 3) Identify the dominant intermolecular forces (dipole-dipole, London dispersion, hydrogen bonding) associated with the following compounds. a) Propane CH3CH CH b) Propanol CH3CH2CH2OH c) PropylChloride CH;CH2CH2Cl Question CCirele the correct answer

Explanation / Answer

Question 2

a)Use ideal gas equation to calculate volume of gas

We know that PV = nRT

V = nRT/P

n = 5 mole,

T = 500C = 50+273.15 = 323.15K,

P= 3 atm,

R = 0.0821 L atm mol-1 K-1 ( R = gas constant)

V = ?

Substitute these value in above equation.

V = 5 X 0.0821 X 323.15 / 3 = 44.22L

volume of 5 mole of Oxygen at 500C and 3 atm pressure = 44.22 liter

b)Use ideal gas equation to calculate volume of gas

We know that PV = nRT

V = nRT/P

n = 10 mole,

T = 500C = 50+273.15 = 323.15K,

P= 3 atm,

R = 0.0821 L atm mol-1 K-1 ( R = gas constant)

V = ?

Substitute these value in above equation.

V = 10 X 0.0821 X 323.15 / 3 = 88.44 L

volume of 10 mole of Oxygen at 500C and 3 atm pressure = 88.44 liter

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