CHEM230P1_06_2014_Y_P1
... Pt(s) | Sn2+ (aq, 0.50 M), Sn4+ (aq, 0.50 M) || I–(aq, 0.15 M) | AgI(s) | Ag(s) ...
... Pt(s) | Sn2+ (aq, 0.50 M), Sn4+ (aq, 0.50 M) || I–(aq, 0.15 M) | AgI(s) | Ag(s) ...
Stoichiometry and the Mole
... If any of the ratios are not a whole number, multiply all the ratios by a factor to make it a whole number – If ratio is ?.5 then multiply by 2; if ?.33 or ?.67 then multiply by 3; if ?.25 or ?.75 then multiply by 4 ...
... If any of the ratios are not a whole number, multiply all the ratios by a factor to make it a whole number – If ratio is ?.5 then multiply by 2; if ?.33 or ?.67 then multiply by 3; if ?.25 or ?.75 then multiply by 4 ...
Final Review 2
... d) None of the above is correct. 61) Which of the following is not one of Dalton’s laws? a) Atoms are indestructible. b) Atoms of the same element have isotopes with different masses. c) Atoms of different elements have different chemical and physical properties. d) All of these are examples of Dalt ...
... d) None of the above is correct. 61) Which of the following is not one of Dalton’s laws? a) Atoms are indestructible. b) Atoms of the same element have isotopes with different masses. c) Atoms of different elements have different chemical and physical properties. d) All of these are examples of Dalt ...
Atom - U of L Class Index
... 2. All of the atoms of a given chemical element are identical in mass and in all other properties. 3. Different elements have different kinds of atoms; these atoms differ in mass from element to element. 4. Atoms are indestructible & retain their identity in all chemical reactions. 5. The formation ...
... 2. All of the atoms of a given chemical element are identical in mass and in all other properties. 3. Different elements have different kinds of atoms; these atoms differ in mass from element to element. 4. Atoms are indestructible & retain their identity in all chemical reactions. 5. The formation ...
Document
... ∆H for making a compound from elements in their standard states Standard state is the most stable form (pure solid, pure liquid, or gas at P = 1 atm) For solutes in solution, standard state is usually 1 M There are tables of ∆Hof ∆Horxn = ∆Hof (products) – ∆Hof (reactants) ...
... ∆H for making a compound from elements in their standard states Standard state is the most stable form (pure solid, pure liquid, or gas at P = 1 atm) For solutes in solution, standard state is usually 1 M There are tables of ∆Hof ∆Horxn = ∆Hof (products) – ∆Hof (reactants) ...
Chemistry Midterm Review Study Guide 2012
... 3. Convert the following word equations into balanced chemical equations: a. Aluminum metal and aqueous copper (II) fluoride yield aqueous aluminum fluoride and solid copper. 2Al (s) + 3CuF2 (aq) 2AlF3(aq) + 3Cu (s) b. Aqueous solutions of sodium chloride and silver nitrate produce an aqueous solu ...
... 3. Convert the following word equations into balanced chemical equations: a. Aluminum metal and aqueous copper (II) fluoride yield aqueous aluminum fluoride and solid copper. 2Al (s) + 3CuF2 (aq) 2AlF3(aq) + 3Cu (s) b. Aqueous solutions of sodium chloride and silver nitrate produce an aqueous solu ...
gram formula mass
... •Matter cannot be created nor destroyed, only changed from one form to another •Energy cannot be created nor destroyed, only changed from one form to another ...
... •Matter cannot be created nor destroyed, only changed from one form to another •Energy cannot be created nor destroyed, only changed from one form to another ...
4 - Quia
... •Matter cannot be created nor destroyed, only changed from one form to another •Energy cannot be created nor destroyed, only changed from one form to another ...
... •Matter cannot be created nor destroyed, only changed from one form to another •Energy cannot be created nor destroyed, only changed from one form to another ...
Chemistry at Karlsruhe 1860
... Laws from Dalton’s Theory Law of conservation of mass – Mass is neither created nor destroyed Law of definite proportion – A given compound always contains exactly the same proportion of elements by mass. ...
... Laws from Dalton’s Theory Law of conservation of mass – Mass is neither created nor destroyed Law of definite proportion – A given compound always contains exactly the same proportion of elements by mass. ...
The Mole
... What if we had 50 moles of hydrogen, how much oxygen would we need and how much water produced? 25 mol O2, 50 mol H2O ...
... What if we had 50 moles of hydrogen, how much oxygen would we need and how much water produced? 25 mol O2, 50 mol H2O ...
2 - C7Chemistry
... The word stoichiometry comes from the Greek words stoicheion which means “element” and metron which means “measure”. ...
... The word stoichiometry comes from the Greek words stoicheion which means “element” and metron which means “measure”. ...
Thermodynamics Enthalpy Entropy and Free Energy Student
... Magnesium flakes were added to an open polystyrene cup filled with 50.0 mL of 1.00 M HCl solution. Assume the specific heat of the solution to be 4.18 J/g°C. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ...
... Magnesium flakes were added to an open polystyrene cup filled with 50.0 mL of 1.00 M HCl solution. Assume the specific heat of the solution to be 4.18 J/g°C. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ...
Final Exam Review
... c. Definite volume; shape of container; no intermolecular attractions d. Volume and shape of container; no intermolecular attractions e. Volume and shape of container; strong intermolecular attractions 102. Which transformation is evaporation? a. liquid ---> solid d. solid ---> gas b. liquid ---> ga ...
... c. Definite volume; shape of container; no intermolecular attractions d. Volume and shape of container; no intermolecular attractions e. Volume and shape of container; strong intermolecular attractions 102. Which transformation is evaporation? a. liquid ---> solid d. solid ---> gas b. liquid ---> ga ...
File
... 1989 A In an experiment to determine the molecular weight and the ionization constant for ascorbic acid (vitamin C), a student dissolved 1.3717 grams of the acid in water to make 50.00 millilitres of solution. The entire solution was titrated with a 0.2211 molar NaOH solution. The pH was monitored t ...
... 1989 A In an experiment to determine the molecular weight and the ionization constant for ascorbic acid (vitamin C), a student dissolved 1.3717 grams of the acid in water to make 50.00 millilitres of solution. The entire solution was titrated with a 0.2211 molar NaOH solution. The pH was monitored t ...
Enthalpy
... Hess’s law states that if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the individual steps. Hess pointed out that the heat absorbed (or evolved) in a given chemical reaction is the same whether the process takes one step or ...
... Hess’s law states that if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the individual steps. Hess pointed out that the heat absorbed (or evolved) in a given chemical reaction is the same whether the process takes one step or ...
Topic 3 MOLE Avodagro`s number = 6.02 x 1023 things = 1 mole 1
... a) How many grams of O2 are needed to burn 1.50 mole of octane? 1.5 mole octane (25mole O2 /2mole octane) (32 g /mole O2) = 600 g 12. One of the steps in the commercial process for converting ammonia to nitric acid involves the conversion of N H3 to NO: 4NH3 (g) + 5 O2 (g) 4NO (g) + 6 H2O (g) In a ...
... a) How many grams of O2 are needed to burn 1.50 mole of octane? 1.5 mole octane (25mole O2 /2mole octane) (32 g /mole O2) = 600 g 12. One of the steps in the commercial process for converting ammonia to nitric acid involves the conversion of N H3 to NO: 4NH3 (g) + 5 O2 (g) 4NO (g) + 6 H2O (g) In a ...
Le Chatelier`s Principle in Iron Thiocyanate Equilibrium
... to relieve or “undo” any stress placed on it. In this case the changes in experimental conditions are the stress. (1) 2 NOCl(g) 2 NO(g) + Cl2(g) H = 75 kJ/mol In the above Equation 1 at equilibrium, if NOCl is added to the system, or if NO or Cl2 is removed the equilibrium will shift to the right ...
... to relieve or “undo” any stress placed on it. In this case the changes in experimental conditions are the stress. (1) 2 NOCl(g) 2 NO(g) + Cl2(g) H = 75 kJ/mol In the above Equation 1 at equilibrium, if NOCl is added to the system, or if NO or Cl2 is removed the equilibrium will shift to the right ...
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.