1 - College of Arts and Sciences
... The states of the reactants and products are written in parentheses to the right of each compound Coefficients are inserted to balance the equation ...
... The states of the reactants and products are written in parentheses to the right of each compound Coefficients are inserted to balance the equation ...
1 - College of Arts and Sciences
... The states of the reactants and products are written in parentheses to the right of each compound Coefficients are inserted to balance the equation ...
... The states of the reactants and products are written in parentheses to the right of each compound Coefficients are inserted to balance the equation ...
Semester 2 Review
... 13. How do you determine actual yield? (Experiment / Calculation) How do you determine theoretical yield? (Experiment / Calculation) Which is generally greater? (Actual / Theoretical) 14. The experimental trial for a reaction produced 13.1 grams of CaO. The stoichiometric calculation showed that 13. ...
... 13. How do you determine actual yield? (Experiment / Calculation) How do you determine theoretical yield? (Experiment / Calculation) Which is generally greater? (Actual / Theoretical) 14. The experimental trial for a reaction produced 13.1 grams of CaO. The stoichiometric calculation showed that 13. ...
Chemical Equations
... • Ca(H2PO4)2 + CaSO4 + HF ---> Ca10F2(PO4)6 + H2SO4 • Typically the arrow is replaced with "produces" or "yields" when the equation is said out loud. • Coefficients are the numbers in front of the formulas. • 2 H2 + O2 ---> 2 H2O • Note the presence of a two in front of the hydrogen and also the wat ...
... • Ca(H2PO4)2 + CaSO4 + HF ---> Ca10F2(PO4)6 + H2SO4 • Typically the arrow is replaced with "produces" or "yields" when the equation is said out loud. • Coefficients are the numbers in front of the formulas. • 2 H2 + O2 ---> 2 H2O • Note the presence of a two in front of the hydrogen and also the wat ...
No Slide Title
... Stoichiometry & Balancing Equations • Remember we stated in the previous chapter that stoichiometry is the study of the quantitative relationships between the amounts of reactants and products in chemical reactions. • We use BALANCED equations to understand stoichiometric relationships of the eleme ...
... Stoichiometry & Balancing Equations • Remember we stated in the previous chapter that stoichiometry is the study of the quantitative relationships between the amounts of reactants and products in chemical reactions. • We use BALANCED equations to understand stoichiometric relationships of the eleme ...
Balancing Equations Notes
... element to count the atoms. Then list the number of atoms of each element on each side. 4. It is often easiest to start balancing with an element that appears only once on each side of the arrow. These elements must have the same coefficient. Next balance elements that appear only once on each side ...
... element to count the atoms. Then list the number of atoms of each element on each side. 4. It is often easiest to start balancing with an element that appears only once on each side of the arrow. These elements must have the same coefficient. Next balance elements that appear only once on each side ...
Chapter 9
... • How many moles of LiOH are required to react with 20 mol of CO2, the average amount exhaled by a person each day? ...
... • How many moles of LiOH are required to react with 20 mol of CO2, the average amount exhaled by a person each day? ...
Chapter 3
... • Methionine, an amino acid used by organisms to make proteins, is represented below. Write the formula for methionine and calculate its molar mass. (red = O; gray = C; blue = N; yellow = S; ivory = H) ...
... • Methionine, an amino acid used by organisms to make proteins, is represented below. Write the formula for methionine and calculate its molar mass. (red = O; gray = C; blue = N; yellow = S; ivory = H) ...
Ch. 8 Notes (Chemical Reactions) Teacher Relearn
... are placed in front of the substances involved Coefficients in the chemical reaction to get the same number of atoms of each element on both sides of the equation. This number will multiply the number of atoms there are in a formula. ...
... are placed in front of the substances involved Coefficients in the chemical reaction to get the same number of atoms of each element on both sides of the equation. This number will multiply the number of atoms there are in a formula. ...
3.4 How do we use the Activity Series
... ADPHS Instructor Ms. Kasia Room 109 UNIT 3 CHEMICAL REACTIONS 3.4 How do we use the Activity Series to Predict if a reaction will take place? AIM: ...
... ADPHS Instructor Ms. Kasia Room 109 UNIT 3 CHEMICAL REACTIONS 3.4 How do we use the Activity Series to Predict if a reaction will take place? AIM: ...
1 - 嘉義大學
... 26. When 3.0 L of hydrogen gas (H2) reacts with 1.0 L of nitrogen gas (N2), 2.0 L of gaseous product are formed. measured at the same temperature and pressure. What is the formula of the product? (A) ...
... 26. When 3.0 L of hydrogen gas (H2) reacts with 1.0 L of nitrogen gas (N2), 2.0 L of gaseous product are formed. measured at the same temperature and pressure. What is the formula of the product? (A) ...
Partial Pressures of Gases
... Let’s examine an equation for the reaction between copper metal and silver nitrate solution. First, we observe metallic copper wire, Cu(s), being immersed in a colourless solution of silver nitrate, AgNO3(aq). The solution gradually changes colour to blue, and sparkling crystals form on the copper w ...
... Let’s examine an equation for the reaction between copper metal and silver nitrate solution. First, we observe metallic copper wire, Cu(s), being immersed in a colourless solution of silver nitrate, AgNO3(aq). The solution gradually changes colour to blue, and sparkling crystals form on the copper w ...
Final
... Be able to determine the oxidation state of elements in a compound Be able to identify the element that is oxidized and the element that is reduced Be able to identify the oxidizing reactant and the reducing reactant. Redox Reactions - Activity series Determine the order of reactivity for a set of e ...
... Be able to determine the oxidation state of elements in a compound Be able to identify the element that is oxidized and the element that is reduced Be able to identify the oxidizing reactant and the reducing reactant. Redox Reactions - Activity series Determine the order of reactivity for a set of e ...
Sample Problems
... 1. Determine the mass of carbon dioxide produced by the decomposition of 50.0 grams of calcium carbonate. 2. Determine the mass of calcium needed to burn in air to produce 14.0 grams of calcium oxide. 3. 60 grams of magnesium ribbon burn in air. a. How many moles of magnesium burns? b. How many mole ...
... 1. Determine the mass of carbon dioxide produced by the decomposition of 50.0 grams of calcium carbonate. 2. Determine the mass of calcium needed to burn in air to produce 14.0 grams of calcium oxide. 3. 60 grams of magnesium ribbon burn in air. a. How many moles of magnesium burns? b. How many mole ...
Practice Problem
... 1. Suppose the mass percents of a compound are 40% carbon, 6.70% hydrogen, and 53.3% oxygen. Determine the empirical formula for this compound. ...
... 1. Suppose the mass percents of a compound are 40% carbon, 6.70% hydrogen, and 53.3% oxygen. Determine the empirical formula for this compound. ...
File
... • In the real world, reactants are not present in the exact mole ratio described by the balanced equation. • This means that one of the reactants will be used up before the other one. – The limiting reactant is used up first and restricts (stops) the reaction – The excess reactant(s) remain after th ...
... • In the real world, reactants are not present in the exact mole ratio described by the balanced equation. • This means that one of the reactants will be used up before the other one. – The limiting reactant is used up first and restricts (stops) the reaction – The excess reactant(s) remain after th ...
Powerpoints - Holy Cross Collegiate
... of reactants and/or products involved in a chemical reaction. • However, the coefficient ratio can only be used to compare amounts of chemicals. • For example, in the formation of carbon dioxide gas, C(s) + O2(g) → CO2(g) it would be correct to say that 1 mol of carbon reacts with 1 mol of oxygen, b ...
... of reactants and/or products involved in a chemical reaction. • However, the coefficient ratio can only be used to compare amounts of chemicals. • For example, in the formation of carbon dioxide gas, C(s) + O2(g) → CO2(g) it would be correct to say that 1 mol of carbon reacts with 1 mol of oxygen, b ...
Chemical Equations & Reactions
... Balancing Chemical Equations • Write a word equation for the reaction. • Write the correct formulas for all reactants and products. • Determine the coefficients that make the equation balance. ...
... Balancing Chemical Equations • Write a word equation for the reaction. • Write the correct formulas for all reactants and products. • Determine the coefficients that make the equation balance. ...
CHM134 General Chemistry I Semester Review – Dr. Steel This list
... 10. What is the mass percent of fluorine in PF5? 11. Balance this equation: C3H8 + O2 Æ CO2 + H2O. What is the coefficient of O2? 12. Calculate the number of molecules in 2.50 grams of CO2. 13. Calculate the mass of 8.60×1024 atoms of Neon, Ne. 14. Balance the equation: P4O10 + H2O Æ H3PO4. How many ...
... 10. What is the mass percent of fluorine in PF5? 11. Balance this equation: C3H8 + O2 Æ CO2 + H2O. What is the coefficient of O2? 12. Calculate the number of molecules in 2.50 grams of CO2. 13. Calculate the mass of 8.60×1024 atoms of Neon, Ne. 14. Balance the equation: P4O10 + H2O Æ H3PO4. How many ...
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.