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What type of loan is IMF's Compensatory and Contingency Financing Facility?
Wiki User
∙ 13y ago
The Compensatory and Contingency Financing Facility is a loan for sudden drops in export earnings.
Wiki User
∙ 13y ago
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Why does propanone has higher vapour pressure than ethanol at room temperature?
The intermolecular forces (IMFs) that attract propane molecules to eachother is far weaker than the IMFs of ethanol molecules. Consequently there is less of an energy barrier for a propane molecule to evaporate. IMFs of propare are limited to the london dispersion forces, which are the weakest IMFs IMFs of ethanol are the london dispersion forces as well as the dipole-dipole interaction (- charge on oxygen and positive on hydrogen) and hydrogen bonding (very strong IMF)
How do you play make you feel my love violin?
To make you feel My Love vijuholin imfs tgo ove dhit
How concentration affect surface tension?
As the strength of intermolecular forces(IMFs) increases, vapor pressure decreases. This is because when IMFs are stronger it is harder for the compound to go to the gas phase, this means that the pressure the compound is exerting on the surrounding environment is lower.
Force of attraction limit the motion of particles most in a solid a liquid a gas both liquid and gas?
The forces are referred to as intermolecular forces, a substances tendency for its molecules to attract to eachother. The stronger these forces are, the more likely a substance will find itself to be solid at room temperature. The reason for this is that the attraction to its own molecules is great enough that the individual particles kinetic energies are not enough to break the intermolecular force. If the IMF is weak, the substance is more likely to be a liquid or even a gas because the attraction to its own molecules is not enough to overcome the particles kinetic energies. In addition the larger a substances chemical structure is, the more surface area available for a molecule to interact and thus the IMFs are stronger, Examples of substances with strong IMFs: Water, NaCl, ethanol, amines Examples of substances with weak IMFs: aliphatic hydrocarbons ( propane ), acetone, ether
What are attractive forces between atoms in molecules?
Atoms are attracted to each other by means of the electromagnetic force. Even though any given atom is electrically neutral (if it isn't, we would call it an ion rather than an atom) it can still have an electromagnetic attraction to another atom, based on the mobility and rearrangements of electrons in their orbits. All electrons repell all other electrons and are attracted to all protons, but they can arrange themselves in such a way as to maximize the attraction and minimize the repulsion.
What type of intermolecular forces exist in Seo2?
Well, SeO2 is a bent molecule. It has 2 lone pairs on the Se central atom, giving it bond angles of 109.5 degrees. Because it's bent, it is polar. We also know (hopefully) that all polar molecules exhibit Dipole-Dipole IMFs. And all molecules exhibit London Dispersion Forces (LDFs). Because it doesn't have any Hydrogen atoms, we can rule out Hydrogen Bonding. So it's just Dipole-dipole and LDFs.
Why do gases failed to obey ideal gas equation at high temperature and low pressure?
You have the idea backwards, gases fail to obey the ideal gas laws at low temperatures and high pressures. The ideal gas law assumes the size of a gas molecule to be negligible as well as the naturally occurring attractive forces between molecules in a gas. These difference diminish when the pressure is low or the temperature is high. Low gas pressure suggests the gas molecules are fairly spaced out, so their individual volumes aren't impeeding the other molecules ability to occupy nearby space. With high pressures gas molecules are forced closer together in order to fit the same amount of volume the greater the volume of individual molecules the less volume available fore gas molecules to occupy. Similarly with high temperatures, the average kinetic energy easily overwhelms the intramolecular forces such as london forces and hydrogen bonding, making their presence almost unimportant. In low temperature applications the imfs of the gas molecules are given much more opportunity to interact as the gas molecules have significantly less kinetic energy.
The type of bonding formed by common elements can be related to their position in the periodic table including bulk properties of their components explain this theory?
I'm not 100% sure what you mean by 'common elements' but I will just try to explain trends in bonding across the periodic table. So, groups 1,2, and Al, Ga, In, Tl, Ge, Sn, Pb, Sb, Bi and Po are all metal so all form metallic bonds the strength of these bond increase as we move across the groups as there are not only more delocalised electrons but also a greater positive nuclear charge. so, the electrons are more attracted to the nucleus. The other group 3 and 4 elements (B, C and Si) form macromolecular or giant covalent structures and covalent bonds as they 3 or 4 outer electrons to share and form a covalent bond with another atom. The many of these strong covalent bonds make these structures strong with high boiling points. From group 5, 6 and 7 the elements form simple a covalent structures as they do not have enough outer electrons to form many bonds. For example take iodine, iodine forms I2. Between the I2 molecules are forces of attraction called van der walls (IMFs). These are weak and are easy to break giving iodine and the other simple covalent molecules low boiling points. Lastly there is, group 0, the noble gases which do not bond (except Xe which can actually bond) so they form simple atomic structures with no covalent bonds and these have very very low boiling points.
