Part-1
... showing negative for which the vapour pressure is minimum. (68% HNO3 + 32% H2O), (20% HCl + 80% H2O). ...
... showing negative for which the vapour pressure is minimum. (68% HNO3 + 32% H2O), (20% HCl + 80% H2O). ...
Covalent Bonding - whitburnscience
... If you know the charge on each of the ions you can easily work out the chemical formula. The way to do this is to cross multiply. So if the negative ions have a charge of 3- and the positive ion a charge of 2+, you simply multiply the positive ion with the 3 and the negative ion with 2, ie X3- Y2+ t ...
... If you know the charge on each of the ions you can easily work out the chemical formula. The way to do this is to cross multiply. So if the negative ions have a charge of 3- and the positive ion a charge of 2+, you simply multiply the positive ion with the 3 and the negative ion with 2, ie X3- Y2+ t ...
Summer Assignment: Some Review / Basic Prep
... Assume all equipment necessary is available to you. You may need to combine methods to achieve a final separation (e.g. dissolving and then filtering out insoluble solids). Your choices are: a) Distillation, because it takes advantage of different boiling points of the liquids in a mixture. b) Elect ...
... Assume all equipment necessary is available to you. You may need to combine methods to achieve a final separation (e.g. dissolving and then filtering out insoluble solids). Your choices are: a) Distillation, because it takes advantage of different boiling points of the liquids in a mixture. b) Elect ...
No Slide Title
... 1. Calculate the standard enthalpy of reaction for the following reaction: 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(l) Hf (NH3) = -132.5 kJ/mol; Hf (NO) = 90.37 kJ/mol; Hf (H2O) = -285.83 kJ/mol 2. Use the enthalpy of combustion of propane gas to calculate the enthalpy of formation of propane gas. C3H ...
... 1. Calculate the standard enthalpy of reaction for the following reaction: 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(l) Hf (NH3) = -132.5 kJ/mol; Hf (NO) = 90.37 kJ/mol; Hf (H2O) = -285.83 kJ/mol 2. Use the enthalpy of combustion of propane gas to calculate the enthalpy of formation of propane gas. C3H ...
First Law of Thermodynamics
... the reactants and products, not on the manner in which they react! This is an important property because it allows us to determine ΔE for a reaction using any path - even one that is unreasonable - as long as the reactants and products remain the same. Both q and w are path dependent, so they are no ...
... the reactants and products, not on the manner in which they react! This is an important property because it allows us to determine ΔE for a reaction using any path - even one that is unreasonable - as long as the reactants and products remain the same. Both q and w are path dependent, so they are no ...
Mechanistic Studies on the Galvanic Replacement Reaction
... For instance, when used as SERS probes or imaging contrast agents, hollow structures of compact sizes would substantially render their accessibility to subcelluar organelles, as well as to speed up their diffusion in tissues.16 Silver nanoparticles <20 nm in size can be prepared as monodispersed sam ...
... For instance, when used as SERS probes or imaging contrast agents, hollow structures of compact sizes would substantially render their accessibility to subcelluar organelles, as well as to speed up their diffusion in tissues.16 Silver nanoparticles <20 nm in size can be prepared as monodispersed sam ...
Revised (12 Sept 2009) Topic: Chemical Equilibrium
... and NCS−(aq) ions (making the denominator bigger). Thus, although both forward and reverse reactions occur simultaneously, the reverse reaction will predominate to decrease the Fe(NCS)2+(aq) concentration until equilibrium is established. When the reverse reaction occurs to a greater extent than the ...
... and NCS−(aq) ions (making the denominator bigger). Thus, although both forward and reverse reactions occur simultaneously, the reverse reaction will predominate to decrease the Fe(NCS)2+(aq) concentration until equilibrium is established. When the reverse reaction occurs to a greater extent than the ...
CHEMISTRY SEC 06 SYLLABUS
... The examination will consist of two written papers, each of two hours’ duration, and an assessment of practical work in chemistry. Questions will be set in English and must be answered in English. The examination will be structured as follows: Paper I consists of a written paper and a practical comp ...
... The examination will consist of two written papers, each of two hours’ duration, and an assessment of practical work in chemistry. Questions will be set in English and must be answered in English. The examination will be structured as follows: Paper I consists of a written paper and a practical comp ...
Type - Enrico Fermi High
... Describe the behavior of the molecules in a liquid. Explain this behavior in terms of intermolecular forces. In a liquid, the molecules can move relatively freely, the intermolecular forces keep them close, but not locked in place. As the intermolecular forces get stronger the molecules are less fre ...
... Describe the behavior of the molecules in a liquid. Explain this behavior in terms of intermolecular forces. In a liquid, the molecules can move relatively freely, the intermolecular forces keep them close, but not locked in place. As the intermolecular forces get stronger the molecules are less fre ...
Chapter 4 Solution Chemistry
... • Many reactions take place in aqueous solution. Water interacts with many substances, and plays an active role in many chemical processes. • Many ionic substances dissolve in water (to at least some extent); water is very good at solvating (dissolving) cations and anions. – The O end of a water mol ...
... • Many reactions take place in aqueous solution. Water interacts with many substances, and plays an active role in many chemical processes. • Many ionic substances dissolve in water (to at least some extent); water is very good at solvating (dissolving) cations and anions. – The O end of a water mol ...
Q - PIMS
... at STP although the sizes and masses of molecules of three gases are very different from each other. Ans: One mole of an ideal gas at S.T.P occupies a volume of 22.414 dm3. Sizes and masses of molecules of different gases do not affect the volume. Normally it is known that in the gaseous state, the ...
... at STP although the sizes and masses of molecules of three gases are very different from each other. Ans: One mole of an ideal gas at S.T.P occupies a volume of 22.414 dm3. Sizes and masses of molecules of different gases do not affect the volume. Normally it is known that in the gaseous state, the ...
Chapter 8 and 9 homework
... analysis to produce 5.77 g CO2 and 2.14 g H20. What is the empirical formula of this compound? 56.Vitamin C is essential for the prevention of scurvy. Combustion of a 2.00 gram sample of this Carbon, Hydrogen and Oxygen containing compound yields 2.998 g CO2 and 0.819 g H20. What is the empirical fo ...
... analysis to produce 5.77 g CO2 and 2.14 g H20. What is the empirical formula of this compound? 56.Vitamin C is essential for the prevention of scurvy. Combustion of a 2.00 gram sample of this Carbon, Hydrogen and Oxygen containing compound yields 2.998 g CO2 and 0.819 g H20. What is the empirical fo ...
Indian Journal of Chemistry
... a variety of synthetic conditions by polymerizing the respective monomers in the presence of silica prepared in situ from an aqueous sodium silicate solution. The composites, thus synthesized, have been characterized by a wide ...
... a variety of synthetic conditions by polymerizing the respective monomers in the presence of silica prepared in situ from an aqueous sodium silicate solution. The composites, thus synthesized, have been characterized by a wide ...
Chapter 14: Chemical Equilibrium
... compare Q and K if Q = K: the system is at equilibrium if Q < K: the system is not at equilibrium the reaction proceeds in the forward direction to reach equilibrium if Q > K: the system is not at equilibrium the reaction proceeds in the reverse direction to reach equilibrium ...
... compare Q and K if Q = K: the system is at equilibrium if Q < K: the system is not at equilibrium the reaction proceeds in the forward direction to reach equilibrium if Q > K: the system is not at equilibrium the reaction proceeds in the reverse direction to reach equilibrium ...
Chapter 19: Thermochemistry II: Entropy and free Energy
... increased, the entropy of a substance increases. The standard entropy of a pure substance, S0, can be determined by careful measurements of the heat capacity as a function of temperature, Cp and by the heat absorbed for each phase change, ∆H0fusion, ∆H0vaporization and ∆H0sublimation. Recall that ...
... increased, the entropy of a substance increases. The standard entropy of a pure substance, S0, can be determined by careful measurements of the heat capacity as a function of temperature, Cp and by the heat absorbed for each phase change, ∆H0fusion, ∆H0vaporization and ∆H0sublimation. Recall that ...
Fall 2002 Honors
... a. (7 pts) She then pushed the plunger half way in and allowed the pump temperature to return to 27°C. What pressure did she read on the pressure gauge? (Remember, there are no air leaks). b. (7 pts) Just after she read that pressure, the phone rang. She dropped the pump and ran to the phone. When s ...
... a. (7 pts) She then pushed the plunger half way in and allowed the pump temperature to return to 27°C. What pressure did she read on the pressure gauge? (Remember, there are no air leaks). b. (7 pts) Just after she read that pressure, the phone rang. She dropped the pump and ran to the phone. When s ...
- Kendriya Vidyalaya NKJ Katni
... 18. 50% of the original amount of a reactant was added to the reaction mixture after 40 min. What % of the total amount will be present after 60 min, given that half life period of the reaction is 20 min. ...
... 18. 50% of the original amount of a reactant was added to the reaction mixture after 40 min. What % of the total amount will be present after 60 min, given that half life period of the reaction is 20 min. ...
(K c ) [A] - Knockhardy
... • from the equation constructed in the first step, write out an expression for Kc. • substitute values from third step and calculate the value of Kc with any units Example 1 One mole of ethanoic acid reacts with one mole of ethanol at 298K. When equilibrium is reached it is found that two thirds of ...
... • from the equation constructed in the first step, write out an expression for Kc. • substitute values from third step and calculate the value of Kc with any units Example 1 One mole of ethanoic acid reacts with one mole of ethanol at 298K. When equilibrium is reached it is found that two thirds of ...
Chapter 3 Stoichiometry
... Stoichiometry is the study of the relationship between relative amounts of substances. The formula of a compound provides information about the relative amount of each element present in either one molecule of the compound or one mole of the compound. For example, one molecule of acetic acid, CH3 ...
... Stoichiometry is the study of the relationship between relative amounts of substances. The formula of a compound provides information about the relative amount of each element present in either one molecule of the compound or one mole of the compound. For example, one molecule of acetic acid, CH3 ...
Thermodynamics of Combustion
... A rich mixture occurs when the quantity of air available is less than the stoichiometric quantity; this means that there is not sufficient air to bum the fuel. In this simplified approach it is assumed that the hydrogen combines preferentially with the oxygen and the carbon does not have sufficient ...
... A rich mixture occurs when the quantity of air available is less than the stoichiometric quantity; this means that there is not sufficient air to bum the fuel. In this simplified approach it is assumed that the hydrogen combines preferentially with the oxygen and the carbon does not have sufficient ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.