CHEMISTRY: Practice Spring Final
... D) 13 kPa 17) Which of the following is not a basic assumption of kinetic theory? A) Gases are composed of particles. B) The particles of all move at the same speed C) The particles of gases are in constant motion. D) All collisions of the gas particles are perfectly elastic. ...
... D) 13 kPa 17) Which of the following is not a basic assumption of kinetic theory? A) Gases are composed of particles. B) The particles of all move at the same speed C) The particles of gases are in constant motion. D) All collisions of the gas particles are perfectly elastic. ...
1 Q. If ΔrH is positive, what can you say about the reaction? 2 Q If
... down (and so its container would get cold) because it is absorbing energy from its surroundings. ...
... down (and so its container would get cold) because it is absorbing energy from its surroundings. ...
2014 Academic Challenge Sectional Chemistry Exam Solution Set 1
... required that this obey a first order rate law or be a gas phase reaction (B or D). The dissociation of chlorine gas into chlorine atoms would be an endothermic reaction due to the bond breaking (C). There are no intermediates in a one-step reaction (E). ...
... required that this obey a first order rate law or be a gas phase reaction (B or D). The dissociation of chlorine gas into chlorine atoms would be an endothermic reaction due to the bond breaking (C). There are no intermediates in a one-step reaction (E). ...
PREP Chemistry 2008 Final Exam Review Problems
... b. Solid aluminum metal reacts with aqueous zinc chloride to produce solid zinc metal and aqueous aluminum chloride. c. Aqueous aluminum sulfate reacts with aqueous barium hydroxide to produce aluminum hydroxide and barium sulfate. Use solubility rules to determine states of products. d. Propane (C3 ...
... b. Solid aluminum metal reacts with aqueous zinc chloride to produce solid zinc metal and aqueous aluminum chloride. c. Aqueous aluminum sulfate reacts with aqueous barium hydroxide to produce aluminum hydroxide and barium sulfate. Use solubility rules to determine states of products. d. Propane (C3 ...
Chapter 8 - profpaz.com
... Mass-Mole Calculations: Relates moles and mass of reactants or products in a balanced chemical equation ...
... Mass-Mole Calculations: Relates moles and mass of reactants or products in a balanced chemical equation ...
Question - Bellingham High School
... the balanced equation, the chemists say that the reactants are in stoichiometric proportions. When this is the case, all the reactants will take part in the reaction and there will be no reactants left over one the reaction is complete. More often than not, one of the reactants is available in limit ...
... the balanced equation, the chemists say that the reactants are in stoichiometric proportions. When this is the case, all the reactants will take part in the reaction and there will be no reactants left over one the reaction is complete. More often than not, one of the reactants is available in limit ...
UNIT 1 - MATTER AND CHEMICAL BONDING
... a) C-12 as basis of mole b) Avogadro’s constant c) isotopic abundance & relative atomic mass d) empirical & molecular formula e) law of definite proportions or constant composition f) quantitative relationships in a balanced equation g) limiting reagent h) actual yield, theoretical yield, percentage ...
... a) C-12 as basis of mole b) Avogadro’s constant c) isotopic abundance & relative atomic mass d) empirical & molecular formula e) law of definite proportions or constant composition f) quantitative relationships in a balanced equation g) limiting reagent h) actual yield, theoretical yield, percentage ...
Name __KEY____________ Per. ______ Polarity and
... If a bond is polar that means that the atoms share their electrons __ unevenly__ (unevenly / evenly), which causes the more electronegative element to have a _ slightly_ (full/ slightly) negative charge and the other to have a slightly _ positive_ (positive/ negative) charge. As the difference in el ...
... If a bond is polar that means that the atoms share their electrons __ unevenly__ (unevenly / evenly), which causes the more electronegative element to have a _ slightly_ (full/ slightly) negative charge and the other to have a slightly _ positive_ (positive/ negative) charge. As the difference in el ...
Chemical Reactions PPT
... Writing and Balancing Chemical Reactions: Common Symbols in Reactions There are other symbols that give scientists additional information about a reaction. – These symbols are used to indicate what kinds of reactants and products are involved, how they react, etc. ...
... Writing and Balancing Chemical Reactions: Common Symbols in Reactions There are other symbols that give scientists additional information about a reaction. – These symbols are used to indicate what kinds of reactants and products are involved, how they react, etc. ...
Unit 7: Chemical Equations & Reactions
... 2. Beginning with that substance, choose an element that appears in only one reactant and one product. • Adjust the coefficients to obtain the same number of atoms of this element on both sides. • Balance polyatomic ions as a unit (if possible). • Re-write H2O as H-OH if hydroxide is present 3. Bala ...
... 2. Beginning with that substance, choose an element that appears in only one reactant and one product. • Adjust the coefficients to obtain the same number of atoms of this element on both sides. • Balance polyatomic ions as a unit (if possible). • Re-write H2O as H-OH if hydroxide is present 3. Bala ...
Chemical Reactions
... gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. ...
... gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. ...
3rd Quarter Test
... c) concentration of the reactants and the products becomes equal d) rates of the opposing reaction becomes equal 20) For a chemical system at equilibrium, a rise in temperature will a) favor the endothermic reaction b) favor the exothermic reaction c) decrease the rates of reaction d) have no effect ...
... c) concentration of the reactants and the products becomes equal d) rates of the opposing reaction becomes equal 20) For a chemical system at equilibrium, a rise in temperature will a) favor the endothermic reaction b) favor the exothermic reaction c) decrease the rates of reaction d) have no effect ...
Chemical reactions cause chemical changes. They involve the
... Question 2: Why do we balance chemical reaction equations? Balancing a chemical reaction equation shows that no matter is created or destroyed. When the equation is balanced there are the same number of atoms of each element on both sides of the arrow. Question 3: What happens to chemical compounds ...
... Question 2: Why do we balance chemical reaction equations? Balancing a chemical reaction equation shows that no matter is created or destroyed. When the equation is balanced there are the same number of atoms of each element on both sides of the arrow. Question 3: What happens to chemical compounds ...
Writing and Classifying Balanced Equations
... Instructions: Examine the following diagrams of molecules performing chemical changes. For each of the examples a. Write the skeleton equation to show each substance as it occurs in the diagrams. Compounds are shown with their atoms touching each other and have a subscript in their chemical formula ...
... Instructions: Examine the following diagrams of molecules performing chemical changes. For each of the examples a. Write the skeleton equation to show each substance as it occurs in the diagrams. Compounds are shown with their atoms touching each other and have a subscript in their chemical formula ...
File - Meissnerscience.com
... A common technique employed by chemists to help them identify the make-up of an unknown substance is the test for percent composition. Experimentally, one can determine the composition by mass of a substance and then convert the mass amounts to percentages. Percent composition for a compound will al ...
... A common technique employed by chemists to help them identify the make-up of an unknown substance is the test for percent composition. Experimentally, one can determine the composition by mass of a substance and then convert the mass amounts to percentages. Percent composition for a compound will al ...
NOTES CHEMICAL REACTIONS:
... reaction (left side of arrow) • Law of Conservation of Mass must be satisfied! ...
... reaction (left side of arrow) • Law of Conservation of Mass must be satisfied! ...
Unit 5 Chemical Properties and Changes Video Notes A ______ is a
... ________________________ A change that alters the identity of a substance resulting in a new substance or substances with different properties ________________________ Those characteristics that can be observed when a chemical reaction changes the identity of the substance, such as potential to rus ...
... ________________________ A change that alters the identity of a substance resulting in a new substance or substances with different properties ________________________ Those characteristics that can be observed when a chemical reaction changes the identity of the substance, such as potential to rus ...
Chemistry2 Midterm Review 2012 – Tuesday
... classify it as heterogeneous or homogeneous. If it is a pure substance, classify it as an element or a compound. a. air b. tomato juice c. iodine crystals d. a nickel e. graphite (carbon) ...
... classify it as heterogeneous or homogeneous. If it is a pure substance, classify it as an element or a compound. a. air b. tomato juice c. iodine crystals d. a nickel e. graphite (carbon) ...
Chem Reactions (and Balancing Equations)
... combines with one of the oxygen atoms from an oxygen molecule (O2) to form H2O. Then, the remaining oxygen atom combines with two more hydrogen atoms (from another H2 molecule) to make a second H2O molecule. ...
... combines with one of the oxygen atoms from an oxygen molecule (O2) to form H2O. Then, the remaining oxygen atom combines with two more hydrogen atoms (from another H2 molecule) to make a second H2O molecule. ...
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.