Respuesta :
Answer:
4.092 kJ
Explanation:
When a material vaporizes, it increases its own energy by absorbing energy from surroundings or a heat source. The specific molar heat of vaporization (kJ/mol) is the energy required to vaporize one mole of a substance. The total energy which can be absorbed by a given amount of material can be determined by multiplying the number of available moles by the specific molar heat of vaporization.
Step 1: Determine number of moles of ethyl chloride in 10.0g
a) Calculate molar mass of ethyl chloride
[tex] C_{2}H_{5}Cl [/tex]
[tex] C = 12g/mol [/tex]
[tex] H = 1g/mol [/tex]
[tex] Cl = 35.5g/mol [/tex]
[tex] molar mass = (C * 2) + (H * 5) + (Cl * 1) [/tex]
[tex] molar mass = (12 * 2) + (1 * 5) + (35.5 * 1) [/tex]
[tex] molar mass = 64.5g/mol [/tex]
b) Divide mass of ethyl chloride by its molar mass to determine 'n', number of moles
[tex] n = \frac{mass}{molar mass} [/tex]
[tex] n = \frac{10.0}{64.5} [/tex]
[tex] n = 0.155mol [/tex]
Step 2: Determine heat removed by available moles of ethyl chloride based on its specific heat of vaporization (v = 26.4 kJ/mol)
[tex] Q = n*v [/tex]
[tex] Q = 0.155*26.4 [/tex]
[tex] Q = 4.092kJ [/tex]
