The Nature of Chemical Reactions
... mass of what you start with has to be equal to the mass of what you end with This is why equations must be balanced!!! A balanced equation says the number of atoms you started with has to be equal to the number of atoms you end with ...
... mass of what you start with has to be equal to the mass of what you end with This is why equations must be balanced!!! A balanced equation says the number of atoms you started with has to be equal to the number of atoms you end with ...
Chemical Reactions - Mr. Brown`s Science Town
... An Intro. To Chemical Reactions What is a chemical reaction? How do we represent chemical reactions? ...
... An Intro. To Chemical Reactions What is a chemical reaction? How do we represent chemical reactions? ...
Balancing Chemical Equations
... the reactants and the chemicals on the right side represent the ...
... the reactants and the chemicals on the right side represent the ...
classification of chemical reactions
... Temperature: an ___________________in temperature _____________________ the rate of chemical reactions (particles move faster, so reaction rate increases) ...
... Temperature: an ___________________in temperature _____________________ the rate of chemical reactions (particles move faster, so reaction rate increases) ...
Answers pg 233 #4,5
... Answers pg 229 #1,2 1 a) Why is the following equation not balanced? N2 + H2 → NH3 Because there are 2 nitrogen atoms on the left side (reactants) and only one nitrogen atom on the right side (products). Also there are 2 hydrogen atoms on the left side (reactants) and 3 hydrogen atoms on the right s ...
... Answers pg 229 #1,2 1 a) Why is the following equation not balanced? N2 + H2 → NH3 Because there are 2 nitrogen atoms on the left side (reactants) and only one nitrogen atom on the right side (products). Also there are 2 hydrogen atoms on the left side (reactants) and 3 hydrogen atoms on the right s ...
Chapter 3 Reading
... •The stoichiometric coefficients in the balanced equation may be interpreted as: •the relative numbers of molecules or formula units involved in the reaction or •the relative numbers of moles involved in the reaction. •The molar quantities given by the coefficients in a balanced equation are called ...
... •The stoichiometric coefficients in the balanced equation may be interpreted as: •the relative numbers of molecules or formula units involved in the reaction or •the relative numbers of moles involved in the reaction. •The molar quantities given by the coefficients in a balanced equation are called ...
CHEMICAL REACTION
... Law of Conservation of Mass. • There will be an equal number of atoms of each element on either side of the equation. ...
... Law of Conservation of Mass. • There will be an equal number of atoms of each element on either side of the equation. ...
AP Chem Stoichiometry Topic#4 Questions WS Name: Date: Per
... (d) Calculate the percent nitrogen by mass in glycine. (3) The diagram is a representation of 20 atoms of a fictitious element, which we will call nevadium (Nv). The red spheres are 293Nv, and the blue spheres are 295Nv. (a) Assuming that this sample is a statistically representative sample of the e ...
... (d) Calculate the percent nitrogen by mass in glycine. (3) The diagram is a representation of 20 atoms of a fictitious element, which we will call nevadium (Nv). The red spheres are 293Nv, and the blue spheres are 295Nv. (a) Assuming that this sample is a statistically representative sample of the e ...
HONORS: UNIT 2B: Antacids Below are the class objectives
... Define and predict products for combustion reactions Product testing - Know the tests for some common products such as oxygen, water, hydrogen and carbon dioxide: burning splint for oxygen, hydrogen or carbon dioxide, and lime water for carbon dioxide. Investigate mass of reactants and products in a ...
... Define and predict products for combustion reactions Product testing - Know the tests for some common products such as oxygen, water, hydrogen and carbon dioxide: burning splint for oxygen, hydrogen or carbon dioxide, and lime water for carbon dioxide. Investigate mass of reactants and products in a ...
Chemical Equations and Reactions
... • Conservation of atoms-the number of each type of atom on the reactants side of the chemical equation MUST be equal to the number of each type of atom on the products side of the equation. • Coefficient-represent the number of units of each substance taking part in the reaction • Balanced chemical ...
... • Conservation of atoms-the number of each type of atom on the reactants side of the chemical equation MUST be equal to the number of each type of atom on the products side of the equation. • Coefficient-represent the number of units of each substance taking part in the reaction • Balanced chemical ...
CHEMISTRY 1 FINAL EXAM REVIEW
... A. a reaction in which a single compound is broken down into simpler substances B. a reaction in which oxygen reacts with another substance, often producing heat or light C. a reaction in which the atoms of one element replace the atoms of a cation in a compound D. a reaction in which two or more su ...
... A. a reaction in which a single compound is broken down into simpler substances B. a reaction in which oxygen reacts with another substance, often producing heat or light C. a reaction in which the atoms of one element replace the atoms of a cation in a compound D. a reaction in which two or more su ...
CHEM_2nd_Semester_Final_R eview
... 4. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 5. The atomic mass unit and the mole are defined using what isotope? 6. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 ...
... 4. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 5. The atomic mass unit and the mole are defined using what isotope? 6. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 ...
Chemistry 2nd Semester Final Exam Review Chemical Bonds Give
... 4. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 5. The atomic mass unit and the mole are defined using what isotope? 6. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 ...
... 4. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 5. The atomic mass unit and the mole are defined using what isotope? 6. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 ...
2nd Semester Final Review
... 4. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 5. The atomic mass unit and the mole are defined using what isotope? 6. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 ...
... 4. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 5. The atomic mass unit and the mole are defined using what isotope? 6. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 ...
Chapter 6
... - The chemical reaction H2(g) + ½ O2(g) → H2O(l) describes the formation of water from its elements. - Butane burns in air to produce carbon dioxide and water: 2C4H10(g) + 13O2 (g) → 2CO2 (g) + 10H2O (g) ...
... - The chemical reaction H2(g) + ½ O2(g) → H2O(l) describes the formation of water from its elements. - Butane burns in air to produce carbon dioxide and water: 2C4H10(g) + 13O2 (g) → 2CO2 (g) + 10H2O (g) ...
FIREWORKS EMC summary notes
... EXAMPLE 1 - The reaction of paraffin with oxygen to form water and carbon dioxide. The reactants are paraffin and oxygen. The products are water and carbon dioxide. ...
... EXAMPLE 1 - The reaction of paraffin with oxygen to form water and carbon dioxide. The reactants are paraffin and oxygen. The products are water and carbon dioxide. ...
09 Stoichiometry WS Stoichiometry WS
... If 1.23 g of lead nitrate are consumed, what is the mass of the potassium nitrate produced? 10. A car battery produces electrical energy with the following chemical reaction: Pb(s) + PbO2(s) + 2H2SO4(aq) 2PbSO4(s) + 2H2O(l) If the battery loses 340. g of lead in this reaction, how many moles of lead ...
... If 1.23 g of lead nitrate are consumed, what is the mass of the potassium nitrate produced? 10. A car battery produces electrical energy with the following chemical reaction: Pb(s) + PbO2(s) + 2H2SO4(aq) 2PbSO4(s) + 2H2O(l) If the battery loses 340. g of lead in this reaction, how many moles of lead ...
Chapter 12 Review “Stoichiometry”
... 0.1 mol of Ca reacts with 880 g water, 2.24 L of hydrogen gas forms (at STP). How would the amount of hydrogen produced change if the volume of water was decreased to 440 mL (440 g)? When two substances react to form products, the reactant which is used up is called the ____. ...
... 0.1 mol of Ca reacts with 880 g water, 2.24 L of hydrogen gas forms (at STP). How would the amount of hydrogen produced change if the volume of water was decreased to 440 mL (440 g)? When two substances react to form products, the reactant which is used up is called the ____. ...
Chapter 12 Review “Stoichiometry”
... 0.1 mol of Ca reacts with 880 g water, 2.24 L of hydrogen gas forms (at STP). How would the amount of hydrogen produced change if the volume of water was decreased to 440 mL (440 g)? When two substances react to form products, the reactant which is used up is called the ____. ...
... 0.1 mol of Ca reacts with 880 g water, 2.24 L of hydrogen gas forms (at STP). How would the amount of hydrogen produced change if the volume of water was decreased to 440 mL (440 g)? When two substances react to form products, the reactant which is used up is called 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.