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final exam review packet
... C- Periodic Table-2301. I can differentiate between groups and periods on the periodic table and what is common about elements within a group. C- Periodic Table-2302. I can locate metals, non-metals and metalloids on the periodic table. C- Periodic Table-2303. I can list properties of metals, non me ...
... C- Periodic Table-2301. I can differentiate between groups and periods on the periodic table and what is common about elements within a group. C- Periodic Table-2302. I can locate metals, non-metals and metalloids on the periodic table. C- Periodic Table-2303. I can list properties of metals, non me ...
g) Chemistry 30 - Mr. Jones LHS Science
... 1. Measure 5 mL of 1.0 M HCl into a test tube. 2. Obtain an equal volume of 1.0 M sodium hydroxide in another test tube. 3. Record the temperature either solution. 4. Pour the NaOH solution into the HCl. Stir and record the highest temperature reached as T2. 5. Discard the solution and clean all mat ...
... 1. Measure 5 mL of 1.0 M HCl into a test tube. 2. Obtain an equal volume of 1.0 M sodium hydroxide in another test tube. 3. Record the temperature either solution. 4. Pour the NaOH solution into the HCl. Stir and record the highest temperature reached as T2. 5. Discard the solution and clean all mat ...
AP CHEMISTRY PROBLEMS ENTHALPY, ENTROPY, AND FREE
... 13. For the reaction 2NO2 (g) ⇆N2O4 (g) , the values of ΔH° and ΔS° are -58.03 kJ and -176.6 J/K respectively. What is the value of ΔG° at 298 K? Assuming that ΔH° and ΔS° do not depend on temperature, at what temperature is ΔG°=O? Is ΔG° negative above or below this ...
... 13. For the reaction 2NO2 (g) ⇆N2O4 (g) , the values of ΔH° and ΔS° are -58.03 kJ and -176.6 J/K respectively. What is the value of ΔG° at 298 K? Assuming that ΔH° and ΔS° do not depend on temperature, at what temperature is ΔG°=O? Is ΔG° negative above or below this ...
IB Chemistry Online EQ_Ans
... b The enthalpy change that occurs when one mole of a pure compound undergoes complete combustion in the presence of excess oxygen under standard conditions.[2] c Hess’s law states that the total enthalpy change for a reaction is independent of the route taken. It depends only on the initial and f ...
... b The enthalpy change that occurs when one mole of a pure compound undergoes complete combustion in the presence of excess oxygen under standard conditions.[2] c Hess’s law states that the total enthalpy change for a reaction is independent of the route taken. It depends only on the initial and f ...
dutch national chemistry olympiad
... 3p 6 Explain by using information from Binas Table 57A that the amount of NO decreases when the gas mixture is cooled down. Mention the numerical value of this information in your explanation. Assume that this information also applies in the conditions present in diesel motors. The temperature of ...
... 3p 6 Explain by using information from Binas Table 57A that the amount of NO decreases when the gas mixture is cooled down. Mention the numerical value of this information in your explanation. Assume that this information also applies in the conditions present in diesel motors. The temperature of ...
! !! ! n nn N P =
... A. Energy can never be created or destroyed but it can be changed from one form to another. B. Two bodies in thermal contact are at thermal equilibrium with each other if the two bodies are at the same absolute temperature. C. Any process carried out in several steps, the overall ∆H is equal to the ...
... A. Energy can never be created or destroyed but it can be changed from one form to another. B. Two bodies in thermal contact are at thermal equilibrium with each other if the two bodies are at the same absolute temperature. C. Any process carried out in several steps, the overall ∆H is equal to the ...
Dalton Model Reading
... chemical compounds; a given compound always has the same relative numbers of types of atoms. 4. Atoms cannot be created, divided into smaller particles, nor destroyed in the chemical process; a chemical reaction simply changes the way atoms are grouped together. 5. Elements are made of tiny particle ...
... chemical compounds; a given compound always has the same relative numbers of types of atoms. 4. Atoms cannot be created, divided into smaller particles, nor destroyed in the chemical process; a chemical reaction simply changes the way atoms are grouped together. 5. Elements are made of tiny particle ...
F Practice Test #2 Solutions
... C) A system that is disturbed from an equilibrium condition responds in such a way as to restore equilibrium. D) Equilibrium in molecular systems is dynamic, with two opposing processes balancing one another. E) A system moves spontaneously toward a state of equilibrium. 11. Which of the following i ...
... C) A system that is disturbed from an equilibrium condition responds in such a way as to restore equilibrium. D) Equilibrium in molecular systems is dynamic, with two opposing processes balancing one another. E) A system moves spontaneously toward a state of equilibrium. 11. Which of the following i ...
國立嘉義大學九十二學年度
... 1.Which pair of elements would be most likely to form an ionic compound? (A) P and Br (B) Cu and K (C) C and O (D) O and Zn (E) Al and Rb 2.According to the solubility rules which one of the following compounds is insoluble in water? (A) NaCl (B) MgBr2 (C) FeCl2 ...
... 1.Which pair of elements would be most likely to form an ionic compound? (A) P and Br (B) Cu and K (C) C and O (D) O and Zn (E) Al and Rb 2.According to the solubility rules which one of the following compounds is insoluble in water? (A) NaCl (B) MgBr2 (C) FeCl2 ...
CHAPTER 4: AQUEOUS REACTIONS AND SOLUTION
... called an electrolyte because it will allow electric current to flow through it. Example: NaCl A substance that does not form ions in solution is called a nonelectrolyte. Example: C12H22O11 ...
... called an electrolyte because it will allow electric current to flow through it. Example: NaCl A substance that does not form ions in solution is called a nonelectrolyte. Example: C12H22O11 ...
Test - Regents
... Setting/Chemistry, and your knowledge of chemistry. In the 1920s, paint used to inscribe the numbers on watch dials was composed of a luminescent (glow-in-the-dark) mixture. The powdered-paint base was a mixture of radium salts and zinc sulfide. As the paint was mixed, the powdered base became airbo ...
... Setting/Chemistry, and your knowledge of chemistry. In the 1920s, paint used to inscribe the numbers on watch dials was composed of a luminescent (glow-in-the-dark) mixture. The powdered-paint base was a mixture of radium salts and zinc sulfide. As the paint was mixed, the powdered base became airbo ...
Study Guide
... 28. If a gas sample is at STP (Standard Temperature and Pressure), what are its temperature and pressure? 29. Calculate the density of oxygen gas (O2) at STP, in g/L. [Use molar mass: O2, 32.0 g/mol] 30. What is the volume (L) occupied by a mole of an ideal gas, if the pressure is 626 mmHg and the t ...
... 28. If a gas sample is at STP (Standard Temperature and Pressure), what are its temperature and pressure? 29. Calculate the density of oxygen gas (O2) at STP, in g/L. [Use molar mass: O2, 32.0 g/mol] 30. What is the volume (L) occupied by a mole of an ideal gas, if the pressure is 626 mmHg and the t ...
PPT - Unit 5
... -(C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(l) ΔH = -1300. kJ) 2( C(s) + O2(g) → CO2(g) ) 2(ΔH = -394 kJ) H2(g) + 1/2O2(g) → H2O(l) ΔH = -286 kJ Calculate ΔH for the following reaction: 2C(s) + H2(g) → C2H2(g) 2C(s) + 2O2(g) → 2CO2(g) ΔH = -788 kJ 2CO2(g) + H2O(l) → C2H2(g) + 5/2O2(g) ΔH = +1300 kJ H2(g) + ...
... -(C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(l) ΔH = -1300. kJ) 2( C(s) + O2(g) → CO2(g) ) 2(ΔH = -394 kJ) H2(g) + 1/2O2(g) → H2O(l) ΔH = -286 kJ Calculate ΔH for the following reaction: 2C(s) + H2(g) → C2H2(g) 2C(s) + 2O2(g) → 2CO2(g) ΔH = -788 kJ 2CO2(g) + H2O(l) → C2H2(g) + 5/2O2(g) ΔH = +1300 kJ H2(g) + ...
Chapter 4 Chemical Quantities and Aqueous
... Assume that while making pizzas, we burn a pizza, drop one on the floor, or other uncontrollable events happen so that we only make two pizzas. The actual amount of product made in a chemical reaction is called the actual yield. We can determine the efficiency of making pizzas by calculating the per ...
... Assume that while making pizzas, we burn a pizza, drop one on the floor, or other uncontrollable events happen so that we only make two pizzas. The actual amount of product made in a chemical reaction is called the actual yield. We can determine the efficiency of making pizzas by calculating the per ...
Chapter 14
... 20. Strategy and Explanation: The two equations are related, so we will use the information in Section 14.2 to identify how their equilibrium constants are related. Multiplying the first equation by a constant factor of 3 gives the second equation. (1) N2H4 (g) + 4/3 ClF3 (g) ' 4 HF (g) + N2 (g) + 2 ...
... 20. Strategy and Explanation: The two equations are related, so we will use the information in Section 14.2 to identify how their equilibrium constants are related. Multiplying the first equation by a constant factor of 3 gives the second equation. (1) N2H4 (g) + 4/3 ClF3 (g) ' 4 HF (g) + N2 (g) + 2 ...
Chem Stoichiometry Study Guide
... 1. ____ Al + ____ O2 ____ Al2O3 2. ____ Cu + ____ AgNO3 ____ Ag + ____ Cu(NO3)2 3. ____ Zn + ____ HCl ____ ZnCl2 + ____ H2 4. ____ Fe + ____ Cl2 ____ FeCl3 PERFORM THE FOLLOWING STOICHIOMETRIC CALCULATIONS: 5. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen. How many ...
... 1. ____ Al + ____ O2 ____ Al2O3 2. ____ Cu + ____ AgNO3 ____ Ag + ____ Cu(NO3)2 3. ____ Zn + ____ HCl ____ ZnCl2 + ____ H2 4. ____ Fe + ____ Cl2 ____ FeCl3 PERFORM THE FOLLOWING STOICHIOMETRIC CALCULATIONS: 5. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen. How many ...
- Catalyst
... 4. The ____________________________ of an element has the units g/mole. 5. Smallest unit of an element is a(n) _________________________________. 6. The __________________________ of an element is one or two letters found on the periodic table. 7. Isotopes have the same number of ____________ ...
... 4. The ____________________________ of an element has the units g/mole. 5. Smallest unit of an element is a(n) _________________________________. 6. The __________________________ of an element is one or two letters found on the periodic table. 7. Isotopes have the same number of ____________ ...
(1/V m C) +
... the radiation. In order for scattering to occur, the plasmon oscillations must be perpendicular to the surface. If they are in plane with the surface, no scattering will occur. It is because of this requirement that roughened surface or arrangements of nanoparticles are typically employed in SERS. ...
... the radiation. In order for scattering to occur, the plasmon oscillations must be perpendicular to the surface. If they are in plane with the surface, no scattering will occur. It is because of this requirement that roughened surface or arrangements of nanoparticles are typically employed in SERS. ...
Final Exam Study Guide Page 1 Quiz
... b. 887.5 moles c. 1.5 x 1025 moles d. none of the above 2. How many grams are in 6.2 moles of NH4? a. .34 g b. 111.8 g c. 6.2 g d. 11.6 g 3. One mole of CaCO3 is equal to how many molecules of CaCO3? a. 765 molecules b. 249 molecules c. 7.6 x 1024 molecules d. 6.02 x 1023 molecules 4. How many grams ...
... b. 887.5 moles c. 1.5 x 1025 moles d. none of the above 2. How many grams are in 6.2 moles of NH4? a. .34 g b. 111.8 g c. 6.2 g d. 11.6 g 3. One mole of CaCO3 is equal to how many molecules of CaCO3? a. 765 molecules b. 249 molecules c. 7.6 x 1024 molecules d. 6.02 x 1023 molecules 4. How many grams ...
Chapter 1 - TamAPChemistryHart
... and a gas C. The gas has exactly the same properties as the product obtained when carbon is burned in an excess of oxygen. Based on these observations, can we determine whether solids A and B and the gas C are elements or compounds? Explain your conclusions for each substance. 16. In the process of ...
... and a gas C. The gas has exactly the same properties as the product obtained when carbon is burned in an excess of oxygen. Based on these observations, can we determine whether solids A and B and the gas C are elements or compounds? Explain your conclusions for each substance. 16. In the process of ...
Colorful Oxidation of Alcohol
... Source: Summerlin, L. R., Borgford, C. L., and Ealy, J. B. (1987) Chemical Demonstrations: A Source Book for Teachers Volume 2. p. 210. Description: When a yellow solution, K2CrO7, is added to three different alcohols, the solution turns blue in two of the alcohols and remains yellow in one. Concept ...
... Source: Summerlin, L. R., Borgford, C. L., and Ealy, J. B. (1987) Chemical Demonstrations: A Source Book for Teachers Volume 2. p. 210. Description: When a yellow solution, K2CrO7, is added to three different alcohols, the solution turns blue in two of the alcohols and remains yellow in one. Concept ...
Redox
![](https://commons.wikimedia.org/wiki/Special:FilePath/NaF.gif?width=300)
Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.