Chapter 5: Thermochemistry
... What is not apparent in the above equation is the role of energy in a reaction. For many reactions, energy, often in the form of heat, is absorbed–that is, it acts somewhat like a reactant. You might write an equation for those reactions that looks like this: Energy + Reactants Products In other r ...
... What is not apparent in the above equation is the role of energy in a reaction. For many reactions, energy, often in the form of heat, is absorbed–that is, it acts somewhat like a reactant. You might write an equation for those reactions that looks like this: Energy + Reactants Products In other r ...
Example of Lab Notebook
... hydrochloride. This was evident as the black oily liquid disappeared upon swirling. This was followed by the addition of 6.3 mL of acetic anhydride which produced some precipitation. Following the addition of an aqueous solution of sodium acetate, the acetanilide product formed much more readily by ...
... hydrochloride. This was evident as the black oily liquid disappeared upon swirling. This was followed by the addition of 6.3 mL of acetic anhydride which produced some precipitation. Following the addition of an aqueous solution of sodium acetate, the acetanilide product formed much more readily by ...
Document
... Avogadro constant of those particles 6.022 x 1023 In 1 mol Na2CO3 , how many… • Na atoms? • C atoms? • O atoms? • How many donuts in 1 mol of donuts? • How many boogers in 1 mol of boogers? Which has more atoms, 1 mol CH3 or 1 mol NH3 ? How about CH3CH2OH or H2SO4 ? ...
... Avogadro constant of those particles 6.022 x 1023 In 1 mol Na2CO3 , how many… • Na atoms? • C atoms? • O atoms? • How many donuts in 1 mol of donuts? • How many boogers in 1 mol of boogers? Which has more atoms, 1 mol CH3 or 1 mol NH3 ? How about CH3CH2OH or H2SO4 ? ...
GCE Getting Started - Edexcel
... assess. Carry out a selection of displacement, precipitation and acid reactions, using mini whiteboards to write equations. Prepare a sample of a salt and compare predicted to actual yield, considering any potential loss of product. Examples could include copper(II) sulfate or ammonium iron(II) sulf ...
... assess. Carry out a selection of displacement, precipitation and acid reactions, using mini whiteboards to write equations. Prepare a sample of a salt and compare predicted to actual yield, considering any potential loss of product. Examples could include copper(II) sulfate or ammonium iron(II) sulf ...
2012 International Practice Exam: Chemistry
... these specific multiple-choice questions at any time in any form with anyone, including your teacher and other students. If you disclose these questions through any means, your AP Exam score will be canceled. Are there any questions? . . . You must complete the answer sheet using a No. 2 pencil only ...
... these specific multiple-choice questions at any time in any form with anyone, including your teacher and other students. If you disclose these questions through any means, your AP Exam score will be canceled. Are there any questions? . . . You must complete the answer sheet using a No. 2 pencil only ...
Final Review 3-8 Answers_2
... 12. A substance was dissolved in water to form a conducting solution that does not affect litmus. This evidence indicates a/an a) acid substance that has ionized in solution b) neutral ionic substance that has dissociated in solution c) base substance that has dissociated in solution d) base substan ...
... 12. A substance was dissolved in water to form a conducting solution that does not affect litmus. This evidence indicates a/an a) acid substance that has ionized in solution b) neutral ionic substance that has dissociated in solution c) base substance that has dissociated in solution d) base substan ...
Higher Chemistry Specimen Question Paper
... (ii) Explain clearly why the first ionisation energy of sodium is much lower than its second ionisation energy. ...
... (ii) Explain clearly why the first ionisation energy of sodium is much lower than its second ionisation energy. ...
sample problem - KFUPM Resources
... The reaction becomes even more spontaneous at the given non standard states since ΔG is more negative than ΔG. Thus, more HCl will be formed with the given pressures. The reaction will continue producing more HCl and consuming more H2 and Cl2 until QP = KP . ...
... The reaction becomes even more spontaneous at the given non standard states since ΔG is more negative than ΔG. Thus, more HCl will be formed with the given pressures. The reaction will continue producing more HCl and consuming more H2 and Cl2 until QP = KP . ...
towards the synthesis of functionalised macrocyclic receptors
... A practical route to the synthesis of two new macrocyclic thio-crown ethers, 13bromo-3,6,9-trithia-15-azabicyclo[9.3.1]pentadeca-1(15),11,13-triene, 82, and 13bromo-3,6,9-trithia-15-azabicyclo[9.3.1]pentadeca-1(15),11,13-triene-15-oxide, 84, is described. Both macrocycles were fully characterised us ...
... A practical route to the synthesis of two new macrocyclic thio-crown ethers, 13bromo-3,6,9-trithia-15-azabicyclo[9.3.1]pentadeca-1(15),11,13-triene, 82, and 13bromo-3,6,9-trithia-15-azabicyclo[9.3.1]pentadeca-1(15),11,13-triene-15-oxide, 84, is described. Both macrocycles were fully characterised us ...
Redox Reactions - Hillsborough County Public Schools
... A compound has an overall charge of zero, which means all the negative charges have to equal the positive charges. Examples: When calculating the oxidation number of N in NO2 , use the rules above to help you. You see that oxygen normally has an oxidation number of -2 and there are two oxygen atoms. ...
... A compound has an overall charge of zero, which means all the negative charges have to equal the positive charges. Examples: When calculating the oxidation number of N in NO2 , use the rules above to help you. You see that oxygen normally has an oxidation number of -2 and there are two oxygen atoms. ...
Experiment 9
... According to the law of equivalents, all the chemicals react with each other in the amounts which are proportional to their chemical equivalents. Chemical equivalent is the amount of a substance (in moles) which can react with 1 mole of hydrogen atoms or replace its same amount from a chemical compo ...
... According to the law of equivalents, all the chemicals react with each other in the amounts which are proportional to their chemical equivalents. Chemical equivalent is the amount of a substance (in moles) which can react with 1 mole of hydrogen atoms or replace its same amount from a chemical compo ...
1. True
... 19.1. Which of the following statements is FALSE? 1. The total amount of energy and matter in the Universe is constant. 2. Breaking chemical bonds is an endothermic process. 3. It is more efficient to use a primary energy source than a secondary energy source. 4. Entropy must be conserved in all che ...
... 19.1. Which of the following statements is FALSE? 1. The total amount of energy and matter in the Universe is constant. 2. Breaking chemical bonds is an endothermic process. 3. It is more efficient to use a primary energy source than a secondary energy source. 4. Entropy must be conserved in all che ...
Chem 1B Fa2015 FinalExam Review
... electronic transition can occur between split 3d subshell, which has energy gap that corresponds to energy of electromagnetic radiation in the visible region; the complex ion [Ni(NH3)6]2+ most probably absorbs in the yellow-orange region; [Zn(NH3)6]2+ is colorless because Zn2+ has [Ar 3d10 configura ...
... electronic transition can occur between split 3d subshell, which has energy gap that corresponds to energy of electromagnetic radiation in the visible region; the complex ion [Ni(NH3)6]2+ most probably absorbs in the yellow-orange region; [Zn(NH3)6]2+ is colorless because Zn2+ has [Ar 3d10 configura ...
Document
... Sample Exercise 5.6 Measuring ΔH Using a Coffee-Cup Calorimeter When a student mixes 50 mL of 1.0 M HCl and 50 mL of 1.0 M NaOH in a coffee-cup calorimeter, the temperature of the resultant solution increases from 21.0 °C to 27.5 °C. Calculate the enthalpy change for the reaction in kJ/mol HCl, ass ...
... Sample Exercise 5.6 Measuring ΔH Using a Coffee-Cup Calorimeter When a student mixes 50 mL of 1.0 M HCl and 50 mL of 1.0 M NaOH in a coffee-cup calorimeter, the temperature of the resultant solution increases from 21.0 °C to 27.5 °C. Calculate the enthalpy change for the reaction in kJ/mol HCl, ass ...
Year Review Booklet (optional)
... Write a balanced chemical equation for each of the following, and classify each as synthesis, decomposition, single replacement, double replacement, neutralization or combustion. a) ...
... Write a balanced chemical equation for each of the following, and classify each as synthesis, decomposition, single replacement, double replacement, neutralization or combustion. a) ...
CHE 1402 Lab Manual
... HCl (be sure NOT to mix CaCO3 and HCl before the experiment). Assemble the apparatus illustrated in Figure 2.1 but do not attach the test tube. Be sure that tube B does not extend below the water level in the bottle. Fill glass tube A and the rubber tubing with water by loosening the pinch clamp and ...
... HCl (be sure NOT to mix CaCO3 and HCl before the experiment). Assemble the apparatus illustrated in Figure 2.1 but do not attach the test tube. Be sure that tube B does not extend below the water level in the bottle. Fill glass tube A and the rubber tubing with water by loosening the pinch clamp and ...
Kinetics Workbook - School District 67
... a) When measuring a property associated with a reactant in a reaction, does it increase or decrease? b) When measuring a property associated with a product in a reaction, does it increase or decrease? Give three ways to measure the rate of the following reaction. State the specific properties that y ...
... a) When measuring a property associated with a reactant in a reaction, does it increase or decrease? b) When measuring a property associated with a product in a reaction, does it increase or decrease? Give three ways to measure the rate of the following reaction. State the specific properties that y ...
Chemistry 211 - George Mason University
... • Matter = physical material of the universe. • Elements = basic building blocks of all other forms of matter. • Atoms = small particles derived from one the elements. All matter can be described in terms of the interactions of atoms with each other. • Molecules (compounds) = combination of two or m ...
... • Matter = physical material of the universe. • Elements = basic building blocks of all other forms of matter. • Atoms = small particles derived from one the elements. All matter can be described in terms of the interactions of atoms with each other. • Molecules (compounds) = combination of two or m ...
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.