A 135 g sample of carbon disulfide requires 43.2 kj of heat to vaporize completely. what is the enthalpy of vaporization for carbon disulfide?
a. 1.77 kj/mol
b. 24.4 kj/mol
c. 76.2 kj/mol
d. 0.320 kj/mol
e. 3.13 kj/mol

Molecular weight of CS2 = 76.14 g

number of moles of CS2 = [tex] \frac{weight.of.CS2}{molecular.weight} [/tex]
= [tex] \frac{135}{76.14} [/tex]
= 1.773

Now, 1.733 mol requires 43.2 kj of heat to vaporize.
∴ 1 mol will require [tex] \frac{43.2}{1.77} [/tex] = 24.4 kj/mol

Thus, correct answer is option B

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A 135 g sample of carbon disulfide requires 43.2 kj of heat to vaporize completely. what is the enthalpy of vaporization for carbon disulfide? a. 1.77 kj/mol b. 24.4 kj/mol c. 76.2 kj/mol d. 0.320 kj/mol e. 3.13 kj/mol

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A 135 g sample of carbon disulfide requires 43.2 kj of heat to vaporize completely. what is the enthalpy of vaporization for carbon disulfide?
a. 1.77 kj/mol
b. 24.4 kj/mol
c. 76.2 kj/mol
d. 0.320 kj/mol
e. 3.13 kj/mol