Since benzene is a covalently bonded chemical, ions and ionic bonds have no bearing on it. Simply put, boiling will cause the molecules to split from one another and turn into a gas.
Benzene boils at a greater temperature than other hydrocarbons with comparable molecular sizes, at 80°C (pentane and hexane, for example). The increased boiling point is most likely caused by how simple it is to create transient dipoles involving the delocalized electrons. At 111°C, methylbenzene begins to boil. Pure benzene and pure toluene have normal boiling points of 80.1 C and 110.6 C, respectively. Due to fewer intermolecular interactions, benzene has a lower boiling point than toluene.
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Changing the volume increases the area that the molecules collide with so the force is spread over a larger area.
Answer:
Above
Explanation:
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To calculate the partial pressure, we have to calulate the total pressure first.
Total pressure = (nRT/V)SO2 + (nRT/V)CO2
n is the number of moles
R is the general gas constant = 0.0821 L.atm/K.mole
T is the temperature in Kelvin
V is the total volume
n SO2 = mass/molar mass = 5/ 32 + 16*2 = 0.078125
n CO2 = mass/molar mass = 5/14+ 16*2 = 0.1
T = 50+273 = 323K
V = 750/1000 = 0.75 liters
Total Pressure = (0.078125*0.0821*323/0.75) + (0.1*0.0821*323/0.75) = 2.7623 + 3.535 = 6.298 atm
Partial pressure = x SO2 * Total Pressure = (no. of moles of SO2 / total no. of moles) * Total pressure = (0.078125/0.078125+0.1) * 6.298 = 2.762 atm.