P1V1=P2V2 3. Explain how your experiment results further prove Boyle’s law. Answer: As the pressure increased, the volume of the gas decreased. When multiplying the pressure change with the volume change, the product was always the same. This further proved Boyle’s Law.
This relationship is specific to the gases that are considered “ideal”. For a gas to be considered “ideal,” it will have no interactions with other molecules and the molecules that make up the gas won’t take up any space. The Ideal Gas Law equation is PV=nRT. “P” stands for pressure, “V” is for volume, “n” gives the number of moles, “R” is the gas constant and “T” is for temperature. The ideal gas constant value is 0.082057 (L x atm)÷(mol x K).
The energy change is the same whether the process occurs in one step or many. Also the first law of thermodynamics which says that energy can be changed from one form to another, but it cannot be created or destroyed. The change in enthalpy (ΔH) determines if energy is absorbed or released by a chemical reaction. Endothermic reactions have a positive value or enthalpy change and are gaining energy, or the reaction can be exothermic which is a negative value or
For purposes of this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is negligible. Even if heat is lost to either of these, it is a fairly constant factor in each part of the experiment, and has little effect on the final results.
A) Subscripts in the reactants must be conserved in the products. B) Coefficients are used to balance the atoms on both sides. C) The law of conservation of matter must be followed. D) Phases are often shown for each compound but are not critical to balancing an equation. E) All of the above statements (a-d) are true.
Molar Volume of a Gas PRE-LAB DISCUSSION Avogadro’s hypothesis states that equal volumes of all gases contain equal numbers of molecules under the same conditions of temperature and pressure. It follows from this hypothesis that all gas samples containing the same number of molecules will occupy the same volume under the same conditions of temperature and pressure. A special name is given to the volume occupied by 1-mole samples of gases at STP. This volume is called the molar volume. In this experiment, you will make an experimental determination of the molar volume.
This is because when an azeotrope is boiled, the resulting vapour has the same ratio of constituents as the original mixture of liquids. Each azeotrope has a characteristic boiling point. The boiling point of an azeotrope is either less than the boiling points of any of its constituents (a positive azeotrope), or greater than the boiling point of any of its constituents (a negative azeotrope). The azeotropes of cyclohexanol/water and cyclohexene/water are both positive azeotropes. The separation of cyclohexene could not depend on distillation alone.
* In heterogeneous equilibria two or more phases are present. * Because the concentrations of pure solids and liquids are constant, these substances are left out of the equilibrium constant expression for a heterogeneous equilibrium. Section 4 * If the concentration of all species in an equilibrium are known, the equilibrium-constant expression can be used to calculate the value of the equilibrium constant. * The changes in the concentrations of reactants and products on the way to achieving equilibrium are governed by the stoichiometry of the reaction. Section 5 * The reaction quotient, Q, is found by substituting reactant and product partial pressures or concentrations into the equilibrium constant
Raoult’s Law was used in this experiment because it describes the vapor pressure that takes place in the experiment. The law states “The vapor pressure of a solution of a non-volatile solute is equal to the vapor pressure of the pure solvent at that temperature multiplied by its mole fraction.” (Clark) This means that the vapor pressure of a solution depends on the vapor pressure of the solutes making up the solvent. Dalton’s Law says that the total vapor pressure of a solution is equal to all of the individual vapor pressures that make up the solution. (Blauch) This law was also used in the lab due to the binary mixture of cyclohexane and toluene. Experimental Section – * Setup fractional distillation equipment * Gathered 7mLof stock mixture * Added four boiling stones
This is due to the fact that pure substances (unlike mixtures) have definite composition. And their components are always the same and are always combined in the same ratio by mass. Because of this, they will always have a constant melting point and boiling point. Follow-Up