Answer:
(a) The molecules begin to move farther apart decreasing their intermolecular forces and they escape the liquid state to enter the gas state.
Explanation:
As we put tea pot full of water on stove the heat transfer starts from surface of tea pot to the closest water molecule near the surface of tea pot, after becoming hot the water rises up and cooler water comes down. When water begins to boil their intermolecular forces begin to decrease and they start to convert in gaseous or vapor state.
The reaction is that,
1 mole is SiCL4 will produce 1 mole of Si(s) Since there is 1 to 1 relationship then we just multiply the enthalpy of reaction by the number of moles
Enthalpy = -625.5 kJ/mole × 12.5 Moles
= -7,818.75 KJ
= -0.78 ×10⁴KJ
If each gas sample has the same temperature and pressure, which has the greatest volume? Since hydrogen gas has the lowest molar mass of the set, 1 g will have the greatest number of moles and therefore the greatest volume. What is the Ideal Gas Law?
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<h3>Answer = 2</h3>
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<h3>Known</h3>
Mass = 32grams
Name of atom = Methane (CH4)
Molar mass C = 12
Molar mass H = 1
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<h3>Question</h3>
molecules (mol?)
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<h3>Way to do</h3>
mass = mol × molar mass
32g = mol × (CH4)
33g = mol × (12 + (4×1))
32g = mol × 16
mol = 32 : 16
mol = 2
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#Ey tell me if its mol or total particles
