For the given O 2 gas in two flasks under same volume and pressure conditions with different temperature condition such that flask A is at 25 o C and flask B at 0 o C , the gas in flask with greater number of O 2 molecules should be determined. Concept introduction: Ideal gas Equation: Any gas can be described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation. V ∝ nT P V = R nT P PV = nRT where, n = moles of gas P = pressure T = temperature R = gas constant Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties. At lower temperature and at high pressures the gas tends to deviate and behave like real gases. Boyle’s Law: At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume. Charles’s Law: At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature. Avogadro’s Hypothesis: Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it. Molar mass: The molar mass of a substance is determined by dividing the given mass of substance by the amount of the substance. Partial pressure: The partial pressure for any gas can be obtained by multiplication of total pressure of the gas with the mole fraction of the gas present in that total mixture. Mole fraction: It defines the amount of particular species present in the mixture. It is obtained by dividing the mole of gas by the total mole of gas present in the mixture.
For the given O 2 gas in two flasks under same volume and pressure conditions with different temperature condition such that flask A is at 25 o C and flask B at 0 o C , the gas in flask with greater number of O 2 molecules should be determined. Concept introduction: Ideal gas Equation: Any gas can be described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation. V ∝ nT P V = R nT P PV = nRT where, n = moles of gas P = pressure T = temperature R = gas constant Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties. At lower temperature and at high pressures the gas tends to deviate and behave like real gases. Boyle’s Law: At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume. Charles’s Law: At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature. Avogadro’s Hypothesis: Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it. Molar mass: The molar mass of a substance is determined by dividing the given mass of substance by the amount of the substance. Partial pressure: The partial pressure for any gas can be obtained by multiplication of total pressure of the gas with the mole fraction of the gas present in that total mixture. Mole fraction: It defines the amount of particular species present in the mixture. It is obtained by dividing the mole of gas by the total mole of gas present in the mixture.
Interpretation: For the given O2 gas in two flasks under same volume and pressure conditions with different temperature condition such that flask A is at 25oC and flask B at 0oC, the gas in flask with greater number of O2 molecules should be determined.
Concept introduction:
Ideal gas Equation:
Any gas can be described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation.
V ∝nTPV = RnTPPV = nRTwhere,n = moles of gasP = pressureT = temperatureR = gas constant
Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties. At lower temperature and at high pressures the gas tends to deviate and behave like real gases.
Boyle’s Law:
At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume.
Charles’s Law:
At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature.
Avogadro’s Hypothesis:
Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it.
Molar mass: The molar mass of a substance is determined by dividing the given mass of substance by the amount of the substance.
Partial pressure: The partial pressure for any gas can be obtained by multiplication of total pressure of the gas with the mole fraction of the gas present in that total mixture.
Mole fraction: It defines the amount of particular species present in the mixture. It is obtained by dividing the mole of gas by the total mole of gas present in the mixture.
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GAY
Organic Reactions Assignment
/26
Write the type of reaction that is occurring on the line provided then complete the reaction. Only include the
major products and any byproducts (e.g. H₂O) but no minor products. Please use either full structural
diagrams or the combination method shown in the lesson. Skeletal/line diagrams will not be accepted.
H3C
1.
2.
CH3
A
Acid
OH
Type of Reaction:
NH
Type of Reaction:
+ H₂O
Catalyst
+ HBr
3.
Type of Reaction:
H3C
4.
Type Reaction:
5. H3C
CH2 + H2O
OH
+
[0]
CH3
Type of Reaction:
6. OH
CH3
HO
CH3 +
Type of Reaction:
7.
Type of Reaction:
+ [H]
humbnai
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Inter Concreting Concentration forms.
Hydrogen peroxide is
a powerful oxidizing agent
wed in concentrated solution in rocket fuels and
in dilute solution as a
hair bleach. An aqueous
sulation of H2O2 is 30% by mass and has
density of #liligime calculat the
Ⓒmolality
⑥mole fraction of
molarity.
20
9.
B. A sample of Commercial Concentrated hydrochloric
ET
If a reaction occurs, what would be the major products? Please include a detailed explanation as well as a drawing showing how the reaction occurs and what the final product is.
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