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Chemical Reactions
... Complete the Do Now via QR code or link I will be about 15-30 min late. This should be completed by the time I arrive. http://bit.ly/1LvB4ak ...
... Complete the Do Now via QR code or link I will be about 15-30 min late. This should be completed by the time I arrive. http://bit.ly/1LvB4ak ...
Section 7.1 Describing Reactions
... © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ...
... © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ...
S2-2-07 - Classifying Chemical Reactions
... synthesis and decomposition reactions. Today we will cover the remainder of the reaction types (single and double displacement and combustion) using discussion, analogy, hands-on experiments, demonstration and work period. ...
... synthesis and decomposition reactions. Today we will cover the remainder of the reaction types (single and double displacement and combustion) using discussion, analogy, hands-on experiments, demonstration and work period. ...
Name______________________ Period________
... d. always equal to the total mass of the products. 66. After the first steps in writing an equation, the equation is balanced by a. adjusting subscripts to the formula(s). b. adjusting coefficients to the smallest whole-number ratio. c. changing the products formed. ...
... d. always equal to the total mass of the products. 66. After the first steps in writing an equation, the equation is balanced by a. adjusting subscripts to the formula(s). b. adjusting coefficients to the smallest whole-number ratio. c. changing the products formed. ...
Chapter 8 Section 1 Describing Chemical Reactions
... Sample Problem E Solution 1. Identify the reactants. Magnesium will attempt to displace lead from lead(II) nitrate. 2. Check the activity series. Magnesium is more active than lead and displaces it. 3. Write the balanced equation. Mg + Pb(NO3)2 Pb + Mg(NO3)2 Double-Displacement Reactions • In a do ...
... Sample Problem E Solution 1. Identify the reactants. Magnesium will attempt to displace lead from lead(II) nitrate. 2. Check the activity series. Magnesium is more active than lead and displaces it. 3. Write the balanced equation. Mg + Pb(NO3)2 Pb + Mg(NO3)2 Double-Displacement Reactions • In a do ...
Chapter 5—Chemical Reactions
... • Balanced chemical equation—the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • Reactions must be balanced to obey the law of conservation of mass. • Coefficients are written to the left of each reactant or product in order to ...
... • Balanced chemical equation—the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • Reactions must be balanced to obey the law of conservation of mass. • Coefficients are written to the left of each reactant or product in order to ...
Review Sheet for Chemistry* First Semester Final
... Chemical reactions can often be classified as one of five types. Write the general form for each type of reaction. Direct Combination (or synthesis): ...
... Chemical reactions can often be classified as one of five types. Write the general form for each type of reaction. Direct Combination (or synthesis): ...
File
... 18. The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia produces __________ g of NO2. A) 2.58 B) 178 C) 119 D) 0.954 19. What are the respective concentrations (M) of Fe3+ and I- afforded by ...
... 18. The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia produces __________ g of NO2. A) 2.58 B) 178 C) 119 D) 0.954 19. What are the respective concentrations (M) of Fe3+ and I- afforded by ...
The Egyptian American International School
... The molar mass of any compound is the mass in grams of one mole of the compound. The molar mass of a compound is the sum of the masses of the component atoms. Percent composition consists of the mass percent of each element in a compound: Mass percent = molar mass of the element X 100 Molar ma ...
... The molar mass of any compound is the mass in grams of one mole of the compound. The molar mass of a compound is the sum of the masses of the component atoms. Percent composition consists of the mass percent of each element in a compound: Mass percent = molar mass of the element X 100 Molar ma ...
quarter 4 final exam guide - District 196 e
... Directions: For each of the following reactant pairs, predict the products that could form when the given reactants are combined. Then write the following in your lab notebook. Balanced molecular equation (include subscripts) Balanced total ionic equation (include subscripts and charges) Net i ...
... Directions: For each of the following reactant pairs, predict the products that could form when the given reactants are combined. Then write the following in your lab notebook. Balanced molecular equation (include subscripts) Balanced total ionic equation (include subscripts and charges) Net i ...
284
... of the combustion of ethyl alcohol, CH5OH, that has been added to the food (perhaps as cognac or rum). C2H5OH(l) + O2(g) CO2(g) + H2O(l) If 25.0 g of ethyl alcohol is burned in air (excess oxygen), calculate the mass of carbon dioxide produced. 33. Small quantities of oxygen gas can be generated i ...
... of the combustion of ethyl alcohol, CH5OH, that has been added to the food (perhaps as cognac or rum). C2H5OH(l) + O2(g) CO2(g) + H2O(l) If 25.0 g of ethyl alcohol is burned in air (excess oxygen), calculate the mass of carbon dioxide produced. 33. Small quantities of oxygen gas can be generated i ...
honors final key
... Mn On catalyst d. + and e. (s) solid f. (g) gas g. (aq) aqueous, in solution, dissolved in water h. (l) liquid ...
... Mn On catalyst d. + and e. (s) solid f. (g) gas g. (aq) aqueous, in solution, dissolved in water h. (l) liquid ...
Chapter 11 Chemical Reactions
... Solid iron (III) sulfide reacts with 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. ...
... Solid iron (III) sulfide reacts with 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. ...
Chemical reactions unit
... 2. An equation can be balanced only by: putting numbers, called coefficients, in front of the chemical formulas. The coefficients tell how many molecules of that compound are present. 3. The numbers of atoms for each element must be the same on each side of the equation. ...
... 2. An equation can be balanced only by: putting numbers, called coefficients, in front of the chemical formulas. The coefficients tell how many molecules of that compound are present. 3. The numbers of atoms for each element must be the same on each side of the equation. ...
Chemical reactions unit
... 1. Determine number of atoms for each element. 2. Pick an element that is not equal on both sides of the equation. 3. Add a coefficient in front of the formula with that element and adjust your counts. 4. Continue adding coefficients to get the same number of atoms of each element on each side. ...
... 1. Determine number of atoms for each element. 2. Pick an element that is not equal on both sides of the equation. 3. Add a coefficient in front of the formula with that element and adjust your counts. 4. Continue adding coefficients to get the same number of atoms of each element on each side. ...
Document
... subscript means that each water molecule has two hydrogen atoms. Since each water molecule has 2 hydrogen atoms and there are two water molecules, there must be 4 (2 × 2) hydrogen atoms. ...
... subscript means that each water molecule has two hydrogen atoms. Since each water molecule has 2 hydrogen atoms and there are two water molecules, there must be 4 (2 × 2) hydrogen atoms. ...
Stoichiometry
![](https://commons.wikimedia.org/wiki/Special:FilePath/Combustion_reaction_of_methane.jpg?width=300)
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.