Lyssa Aruda Writ 340 Dr. Ramsey 1 May 2013 Recipe for Success
... and Na2CO3 are both salts containing polyatomic ions. In aqueous solutions, they separate into their separate ions, Na+, HCO3-, and CO32-. If we include the acid in the original balanced equation, the reaction can be written as NaHCO3 + H+ Na+ + H2O + CO2. Looking at this equation, Na+ appears in ...
... and Na2CO3 are both salts containing polyatomic ions. In aqueous solutions, they separate into their separate ions, Na+, HCO3-, and CO32-. If we include the acid in the original balanced equation, the reaction can be written as NaHCO3 + H+ Na+ + H2O + CO2. Looking at this equation, Na+ appears in ...
Chapter 4 Power Point Quiz
... How many grams of glucose (C6H12O6) form when 4.40 g of CO2 react? a) b) c) d) ...
... How many grams of glucose (C6H12O6) form when 4.40 g of CO2 react? a) b) c) d) ...
How does it vary with the charge and distance of the ions?
... b) Find out the ground state term symbols for boron (z=5) c) Give the significance of magnetic Q.N. d) Show that the Plank’s constant and the angular momentum have the same dimension. e) In the ground state H-atom, the total energy of the electron is -13.6ev. Determine its kinetic energy and potenti ...
... b) Find out the ground state term symbols for boron (z=5) c) Give the significance of magnetic Q.N. d) Show that the Plank’s constant and the angular momentum have the same dimension. e) In the ground state H-atom, the total energy of the electron is -13.6ev. Determine its kinetic energy and potenti ...
key for Unit 1 pp 21
... (c) Cadaverine is a molecular compound formed in decomposing fish. It has a molar mass of 102.18 and is composed solely of C, H, and N. When 0.03560 g of cadaverine is combusted in an excess of oxygen, 0.07665 g of CO2 and 0.04392 g of H2O are formed. What are the simplest formula and molecular form ...
... (c) Cadaverine is a molecular compound formed in decomposing fish. It has a molar mass of 102.18 and is composed solely of C, H, and N. When 0.03560 g of cadaverine is combusted in an excess of oxygen, 0.07665 g of CO2 and 0.04392 g of H2O are formed. What are the simplest formula and molecular form ...
Uses of Sulfuric Acid
... Waste products Most of the “waste” heat is recovered and used to heat water, in this way much of the energy can be reused. Because of this many sulfuric acid plants are co-located with other industrial processes. Great care needs to be taken with the waste gases that are formed. There will be small ...
... Waste products Most of the “waste” heat is recovered and used to heat water, in this way much of the energy can be reused. Because of this many sulfuric acid plants are co-located with other industrial processes. Great care needs to be taken with the waste gases that are formed. There will be small ...
CHAPTER-7
... Ans. It is an equilibrium in which all the reactants and products are in same phase. Example: H2(g)+I2(g) 2HI(g) 9) What is heterogeneous equilibrium? given an example Ans. It is an equilibrium in which reactants and products are in different phases. Example: CaCO3(s) CaO(s) +CO2 (g) 10) State l ...
... Ans. It is an equilibrium in which all the reactants and products are in same phase. Example: H2(g)+I2(g) 2HI(g) 9) What is heterogeneous equilibrium? given an example Ans. It is an equilibrium in which reactants and products are in different phases. Example: CaCO3(s) CaO(s) +CO2 (g) 10) State l ...
CHAPTER 21 NONMETALLIC ELEMENTS AND THEIR COMPOUNDS
... The density of a gas depends on temperature, pressure, and the molar mass of the substance. When two gases are at the same pressure and temperature, the ratio of their densities should be the same as the ratio of their molar masses. The molar mass of ammonium chloride is 53.5 g/mol, and the ratio of ...
... The density of a gas depends on temperature, pressure, and the molar mass of the substance. When two gases are at the same pressure and temperature, the ratio of their densities should be the same as the ratio of their molar masses. The molar mass of ammonium chloride is 53.5 g/mol, and the ratio of ...
Lab 13
... 2. Which of the following rankings correctly shows the order of increasing acidity for benzoic acid, benzensulfonic acid, ethanol and phenol? __A. phenol < ethanol < benzoic acid < benzenesulfonic acid __B. ethanol < phenol < benzenesulfonic acid < benzoic acid __C. ethanol < phenol < benzoic acid < ...
... 2. Which of the following rankings correctly shows the order of increasing acidity for benzoic acid, benzensulfonic acid, ethanol and phenol? __A. phenol < ethanol < benzoic acid < benzenesulfonic acid __B. ethanol < phenol < benzenesulfonic acid < benzoic acid __C. ethanol < phenol < benzoic acid < ...
Changes in Matter: Physical and Chemical Changes
... as a color change, most chemical changes are not visible. A change in matter that produces one or more new substances is called a chemical change, or a chemical reaction. In some chemical changes, a single substance simply changes to one or more substances. In other chemical changes, two or more sub ...
... as a color change, most chemical changes are not visible. A change in matter that produces one or more new substances is called a chemical change, or a chemical reaction. In some chemical changes, a single substance simply changes to one or more substances. In other chemical changes, two or more sub ...
chemistry writing team
... Law of conservation of mass : ‘Mass can neither be created nor destroyed.’ In all physical and chemical changes, the total mass of reactants is equal to that of products. Law of constant composition : A chemical compound is always found to be made of same elements combined together in the same fixed ...
... Law of conservation of mass : ‘Mass can neither be created nor destroyed.’ In all physical and chemical changes, the total mass of reactants is equal to that of products. Law of constant composition : A chemical compound is always found to be made of same elements combined together in the same fixed ...
Chemical Equilibrium - Chemistry with Mrs. Caruso Let the Bonding
... Kp- _partial pressures__are used in the calculation of this equilibrium. Relationship between Kp and Kc: Based on the ideal gas law: Therefore, Kp = Kc(RT)∆n Ex. At 327°C, the equilibrium concentrations are [CH3OH]= .15M, [CO]= .24M, and [H2]=1.1M for the reaction CH3OH (g) ⇌ CO (g) + 2H2 (g) Calcul ...
... Kp- _partial pressures__are used in the calculation of this equilibrium. Relationship between Kp and Kc: Based on the ideal gas law: Therefore, Kp = Kc(RT)∆n Ex. At 327°C, the equilibrium concentrations are [CH3OH]= .15M, [CO]= .24M, and [H2]=1.1M for the reaction CH3OH (g) ⇌ CO (g) + 2H2 (g) Calcul ...
SOLVING L-L EXTRACTION PROBLEMS WITH EXCEL
... numerical solution with a spreadsheet. This is one of the main reasons why L-L extraction analysis is usually performed on a graphical diagram. Hence, to solve the problem numerically, it is necessary to establish a mathematical relationship of equilibrium compositions. Users of Excel will be tempte ...
... numerical solution with a spreadsheet. This is one of the main reasons why L-L extraction analysis is usually performed on a graphical diagram. Hence, to solve the problem numerically, it is necessary to establish a mathematical relationship of equilibrium compositions. Users of Excel will be tempte ...
Descriptive Chemistry for Midterm Exam #2
... Occurrence: found in more compounds than any other element on earth. It is the most abundant element in universe. Oxidation states: 0 in H2, +1 in compounds with other non-metals, −1 in metal hydrides. Industrial Preparation of H2: This is carried out through the reduction of +1 oxidation state in H ...
... Occurrence: found in more compounds than any other element on earth. It is the most abundant element in universe. Oxidation states: 0 in H2, +1 in compounds with other non-metals, −1 in metal hydrides. Industrial Preparation of H2: This is carried out through the reduction of +1 oxidation state in H ...
Equilibrium Booklet - mrstorie
... d) increasing the volume of the container. e) adding a catalyst. 2. For the reaction: CH4(g) + H2O(g) + 49.3 kJ CO(g) + 3 H2(g) Predict the effect on the position of the equilibrium that results from a) increasing temperature. b) decreasing temperature. c) decreasing the pressure. d) decreasing t ...
... d) increasing the volume of the container. e) adding a catalyst. 2. For the reaction: CH4(g) + H2O(g) + 49.3 kJ CO(g) + 3 H2(g) Predict the effect on the position of the equilibrium that results from a) increasing temperature. b) decreasing temperature. c) decreasing the pressure. d) decreasing t ...
H2-rich fluids from serpentinization: Geochemical and biotic
... buffer metamorphic fluids to extremely reducing conditions that are capable of producing hydrogen gas. Awaruite, FeNi3, forms early in this process when the serpentinite minerals are Fe-rich. Olivine with the current mantle Fe兾Mg ratio was oxidized during serpentinization after the Moon-forming impa ...
... buffer metamorphic fluids to extremely reducing conditions that are capable of producing hydrogen gas. Awaruite, FeNi3, forms early in this process when the serpentinite minerals are Fe-rich. Olivine with the current mantle Fe兾Mg ratio was oxidized during serpentinization after the Moon-forming impa ...
Chapter 3 HWsolutions (from Handout)
... Remember, an empirical formula tells us which elements are present and the simplest whole-number ratio of their atoms. This ratio is also a mole ratio. Let nC, nH, nO, nN, and nNa be the number of moles of elements present. Use the molar masses of these elements as conversion factors to convert to m ...
... Remember, an empirical formula tells us which elements are present and the simplest whole-number ratio of their atoms. This ratio is also a mole ratio. Let nC, nH, nO, nN, and nNa be the number of moles of elements present. Use the molar masses of these elements as conversion factors to convert to m ...
Calculations on the equations reaction
... Determine the degree of oxidation of elements. Write the oxidant and reductant. 20.To equalize the oxidation-reduction reaction by electron balance method KMnO4 + HCl → MnCl2 + H2O +Cl2 + KCl . Determine the degree of oxidation of elements. Write the oxidant and reductant. Calculations based on the ...
... Determine the degree of oxidation of elements. Write the oxidant and reductant. 20.To equalize the oxidation-reduction reaction by electron balance method KMnO4 + HCl → MnCl2 + H2O +Cl2 + KCl . Determine the degree of oxidation of elements. Write the oxidant and reductant. Calculations based on the ...
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.