+ H 2 (g)
... (g) if: any “big 7” , CO2, CO. (aq) if: all acids, dissolved in water, solution. electric if electricity is added. *If substance does not fit above criteria, do not put any state of matter. ...
... (g) if: any “big 7” , CO2, CO. (aq) if: all acids, dissolved in water, solution. electric if electricity is added. *If substance does not fit above criteria, do not put any state of matter. ...
CHE 145-381 – TEST #2 SPRING 2009 CHAPTERS 6, 7, 8 NAME
... You may use the Periodic Table. Please note that all quantities needed for the successful completion of this test have been given. Feel free to ask questions for clarification. 1. Indicate to which of the following types of chemical reactions each of the statements listed applies: synthesis, decompo ...
... You may use the Periodic Table. Please note that all quantities needed for the successful completion of this test have been given. Feel free to ask questions for clarification. 1. Indicate to which of the following types of chemical reactions each of the statements listed applies: synthesis, decompo ...
Worksheet
... Coefficients - the numbers written in front of the chemical formulas. You wrote coefficients when you balanced equations. Reactants - the elements or compounds on the left hand side of the equation before the are known as the reactants. Products - the elements or compounds on the right side of the ...
... Coefficients - the numbers written in front of the chemical formulas. You wrote coefficients when you balanced equations. Reactants - the elements or compounds on the left hand side of the equation before the are known as the reactants. Products - the elements or compounds on the right side of the ...
Lab Stuff
... Big Ideas: 1. Ionic compounds form when atoms gain or lose electrons. Metals lose electrons, nonmetals gain them. 2. The number of electrons gained or lost can be predicted with an understanding of the octet rule and the number of valence electrons an atom contains. 3. The periodic table is organize ...
... Big Ideas: 1. Ionic compounds form when atoms gain or lose electrons. Metals lose electrons, nonmetals gain them. 2. The number of electrons gained or lost can be predicted with an understanding of the octet rule and the number of valence electrons an atom contains. 3. The periodic table is organize ...
Balancing a Chemical Equation
... MUST ALSO BE FOLLOWED! Energy changes are written in (endo-/ exothermic reactions) ...
... MUST ALSO BE FOLLOWED! Energy changes are written in (endo-/ exothermic reactions) ...
Balancing a Chemical Equation
... MUST ALSO BE FOLLOWED! Energy changes are written in (endo-/ exothermic reactions) ...
... MUST ALSO BE FOLLOWED! Energy changes are written in (endo-/ exothermic reactions) ...
PDF
... numerous causes. Some materials are lost during transfers from one container to another and side reactions take place that are different from the one that is intended to take place. • The amount of product calculated in the examples is called the theoretical yield. The amount of product actually pro ...
... numerous causes. Some materials are lost during transfers from one container to another and side reactions take place that are different from the one that is intended to take place. • The amount of product calculated in the examples is called the theoretical yield. The amount of product actually pro ...
PPT
... • A balanced chemical equation is one in which the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • A reaction can be balanced by applying the law of conservation of matter. • Coefficients (in red below) are written to the left ...
... • A balanced chemical equation is one in which the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • A reaction can be balanced by applying the law of conservation of matter. • Coefficients (in red below) are written to the left ...
1st Semester Exam in High School Chemistry
... 52. Baking soda (sodium bicarbonate) is a compound commonly used in baked goods, as a deodorizer in refrigerators and as an antacid. Commercial quantities of baking soda are produced by mixing soda ash dissolved in water with carbon dioxide. Baking soda precipitates as a solid from this method: Na2 ...
... 52. Baking soda (sodium bicarbonate) is a compound commonly used in baked goods, as a deodorizer in refrigerators and as an antacid. Commercial quantities of baking soda are produced by mixing soda ash dissolved in water with carbon dioxide. Baking soda precipitates as a solid from this method: Na2 ...
Chemistry- CST Review
... b) 25.2 g of potassium nitrate, KNO3, in enough water to make 150.0 mL of solution. 5. Calculate the number of grams of solute needed to prepare each of the following solutions: a) 4500.0 mL of a 2.0M solution of potassium hydroxide, KOH. b) 2.0 liters of 3.0M nitric acid, HNO3, solution. ...
... b) 25.2 g of potassium nitrate, KNO3, in enough water to make 150.0 mL of solution. 5. Calculate the number of grams of solute needed to prepare each of the following solutions: a) 4500.0 mL of a 2.0M solution of potassium hydroxide, KOH. b) 2.0 liters of 3.0M nitric acid, HNO3, solution. ...
2014-15 FINAL REVIEW Nomenclature: Chemical Name Chemical
... 4. How many moles of gas are in a 30 liter scuba canister if the temperature of the canister is 300 K and the pressure is 200 atmospheres? 5. What’s the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of nitrogen, and 1 mole of hydrogen and has a tota ...
... 4. How many moles of gas are in a 30 liter scuba canister if the temperature of the canister is 300 K and the pressure is 200 atmospheres? 5. What’s the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of nitrogen, and 1 mole of hydrogen and has a tota ...
balancing eqns teacher
... MUST ALSO BE FOLLOWED! Energy changes are written in (endo-/ exothermic reactions) ...
... MUST ALSO BE FOLLOWED! Energy changes are written in (endo-/ exothermic reactions) ...
physics - Keith E. Holbert
... • isotope: nuclides with equal number of protons, but different numbers of neutrons • isotone: nuclides with equal number of neutrons, but different number of protons • isobars: nuclides with same total number of protons and neutrons, different combinations of Z & N • element (particular Z, any N) v ...
... • isotope: nuclides with equal number of protons, but different numbers of neutrons • isotone: nuclides with equal number of neutrons, but different number of protons • isobars: nuclides with same total number of protons and neutrons, different combinations of Z & N • element (particular Z, any N) v ...
percent composition and formulas
... left side and the correct formula(s) for the product(s) on the right side of the equation. Ethane reacts with oxygen to form carbon dioxide and water C2H6 + O2 ...
... left side and the correct formula(s) for the product(s) on the right side of the equation. Ethane reacts with oxygen to form carbon dioxide and water C2H6 + O2 ...
Chapter 19 Reaction Rates And Equilibrium
... • Particles of reactants (ions, atoms, molecules) must collide in order for reactions to occur • An effective collision occurs when reactant particles approach each other: – at the proper angle – With enough Energy (Force) ...
... • Particles of reactants (ions, atoms, molecules) must collide in order for reactions to occur • An effective collision occurs when reactant particles approach each other: – at the proper angle – With enough Energy (Force) ...
Final Review 2006
... d. change in total mass of substances ____ 31. A solid produced by a chemical reaction in solution that separates from the solution is called a. a precipitate. c. a molecule. b. a reactant. d. the mass of the product. ____ 32. After the correct formula for a reactant in an equation has been written, ...
... d. change in total mass of substances ____ 31. A solid produced by a chemical reaction in solution that separates from the solution is called a. a precipitate. c. a molecule. b. a reactant. d. the mass of the product. ____ 32. After the correct formula for a reactant in an equation has been written, ...
Chemical Reactions
... “Yields,” separates reactants from products Used in place of for reversible reactions ...
... “Yields,” separates reactants from products Used in place of for reversible reactions ...
Learning Guide – Poisons (I)
... Meat turns brown when you cook it. Plants make sugar and oxygen from carbon dioxide and water. “Hot hands” get warm when bent. Old wine turns into vinegar. Paint remover loosens paint so it can be removed. Balancing chemical reactions When we write a chemical reaction, it is important to know how ma ...
... Meat turns brown when you cook it. Plants make sugar and oxygen from carbon dioxide and water. “Hot hands” get warm when bent. Old wine turns into vinegar. Paint remover loosens paint so it can be removed. Balancing chemical reactions When we write a chemical reaction, it is important to know how ma ...
(the products). Mass is conserved in a chemical reaction
... atoms are conserved. Subscripts are never changed. • For example when the number of atoms of the reactant element(s) are the same as the number of atoms of the product element(s), the equation is balanced. ...
... atoms are conserved. Subscripts are never changed. • For example when the number of atoms of the reactant element(s) are the same as the number of atoms of the product element(s), the equation is balanced. ...
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... side of the arrow (and also the number of oxygen atoms on the left side of the arrow), equals the number of hydrogen atoms (and likewise the number of oxygen atoms), on the right side of the arrow. Atoms are the smallest units of matter that retain chemical properties. Atoms are not visible under n ...
... side of the arrow (and also the number of oxygen atoms on the left side of the arrow), equals the number of hydrogen atoms (and likewise the number of oxygen atoms), on the right side of the arrow. Atoms are the smallest units of matter that retain chemical properties. Atoms are not visible under n ...
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.