Chemistry I Exams and Answer Keys 2015 Season
... test tube filled with dilute hydrochloric acid, the metal soon floats to the surface of the liquid. The density of magnesium is 1.79 g·cm–3, and the density of the HCl solution is 1.048 g·cm–3. The best explanation for the metal floating on the liquid is that A. the metal is less dense than the acid ...
... test tube filled with dilute hydrochloric acid, the metal soon floats to the surface of the liquid. The density of magnesium is 1.79 g·cm–3, and the density of the HCl solution is 1.048 g·cm–3. The best explanation for the metal floating on the liquid is that A. the metal is less dense than the acid ...
Practice Test 11 - U of L Class Index
... A chunk of white phosphorus weighing 6.58 grams is put in a 750 mL flask containing dry argon (which is then removed using a vacuum, leaving only the phosphorus in the flask). A separate 750 mL flask contains 3.15 bar of fluorine gas (at 19.65 °C). The two flasks are connected so that the two compou ...
... A chunk of white phosphorus weighing 6.58 grams is put in a 750 mL flask containing dry argon (which is then removed using a vacuum, leaving only the phosphorus in the flask). A separate 750 mL flask contains 3.15 bar of fluorine gas (at 19.65 °C). The two flasks are connected so that the two compou ...
Name - cloudfront.net
... The shape of the methane molecule (CH4) is called ____. What is a typical characteristic of an ionic compound? What causes hydrogen bonding? According to the VSEPR theory, molecules adjust their shapes to keep ____ as far apart as possible. Which of the following atoms acquires the most negative cha ...
... The shape of the methane molecule (CH4) is called ____. What is a typical characteristic of an ionic compound? What causes hydrogen bonding? According to the VSEPR theory, molecules adjust their shapes to keep ____ as far apart as possible. Which of the following atoms acquires the most negative cha ...
Honors Chemistry Review Packet KEY
... the same set of intensive properties because they have different chemical compositions. 12. As either heterogeneous or homogeneous 13. Differences in physical properties 15. a) homogeneous, b) heterogeneous, c) homogeneous, d) heterogeneous 21. The liquid was not an element because a solid was lefto ...
... the same set of intensive properties because they have different chemical compositions. 12. As either heterogeneous or homogeneous 13. Differences in physical properties 15. a) homogeneous, b) heterogeneous, c) homogeneous, d) heterogeneous 21. The liquid was not an element because a solid was lefto ...
CHEM 1305 - HCC Learning Web
... D)6-------11. The compound H2O is classified as which of the following? A) Binary ionic B) Ternary ionic C) Binary molecular D) Binary acid -------12. What is the term for a single atom bearing a positive or a negative charge as the result of gaining or losing valence electrons? A) Anion B) Cation C ...
... D)6-------11. The compound H2O is classified as which of the following? A) Binary ionic B) Ternary ionic C) Binary molecular D) Binary acid -------12. What is the term for a single atom bearing a positive or a negative charge as the result of gaining or losing valence electrons? A) Anion B) Cation C ...
File
... Chemists generally refer to the energy given out when a fuel burns in kJmol-1 because this compares the same number of molecules of each fuel. For use as fuels it is sometimes better to convert the units from kJmol-1 to kJg-1 (OR the energy density) of a fuel ...
... Chemists generally refer to the energy given out when a fuel burns in kJmol-1 because this compares the same number of molecules of each fuel. For use as fuels it is sometimes better to convert the units from kJmol-1 to kJg-1 (OR the energy density) of a fuel ...
1. formulae equations and amount
... acid in the stomach or acid spills because they are not corrosive and will not cause a hazard if used in excess. They also have no toxicity if used for indigestion remedies but the CO2 produced can cause wind. Magnesium hydroxide is also suitable for dealing with excess stomach acid as it has low so ...
... acid in the stomach or acid spills because they are not corrosive and will not cause a hazard if used in excess. They also have no toxicity if used for indigestion remedies but the CO2 produced can cause wind. Magnesium hydroxide is also suitable for dealing with excess stomach acid as it has low so ...
WELCOME TO AP CHEMISTRY
... 41. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide? Pb(NO3)2(aq) + NaOH(aq) ----> Pb(OH)2(s) + NaNO3(aq) (unbalanced) ...
... 41. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide? Pb(NO3)2(aq) + NaOH(aq) ----> Pb(OH)2(s) + NaNO3(aq) (unbalanced) ...
Chemistry 12 Keq WORKSHEET #1
... A reaction vessel with a capacity of 1.0 litre, in which the following reaction : SO2 (g) + NO2 (g) <===> SO3 (g) + NO (g) had reached a state of equilibrium, was found to contain 0.40 moles of SO3 , 0.30 moles of NO, 0.15 moles of NO2 , and 0.20 moles of SO2. Calculate the equilibrium constant for ...
... A reaction vessel with a capacity of 1.0 litre, in which the following reaction : SO2 (g) + NO2 (g) <===> SO3 (g) + NO (g) had reached a state of equilibrium, was found to contain 0.40 moles of SO3 , 0.30 moles of NO, 0.15 moles of NO2 , and 0.20 moles of SO2. Calculate the equilibrium constant for ...
2nd Semester Chemistry Terms - Glancy 4TH PERIOD PHYSICAL
... understanding of how the natural world operates 41. Applied research- a branch of scientific research that focuses on developing applications built upon the principles discovered through basic research 42. Molecule- a submicroscopic particle consisting of a group of atoms 43. Submicroscopic- refers ...
... understanding of how the natural world operates 41. Applied research- a branch of scientific research that focuses on developing applications built upon the principles discovered through basic research 42. Molecule- a submicroscopic particle consisting of a group of atoms 43. Submicroscopic- refers ...
H2, N2, O2, F2, Cl2, Br2, I2
... atom we have in the balanced equation. If there is no number in front, a " 1 " is there but we usually leave out the 1's. • Do not change subscripts to balance. They are part of the molecular formula. • States of matter may or may not be included and are not used in balancing. They just tell us a li ...
... atom we have in the balanced equation. If there is no number in front, a " 1 " is there but we usually leave out the 1's. • Do not change subscripts to balance. They are part of the molecular formula. • States of matter may or may not be included and are not used in balancing. They just tell us a li ...
Ionic Equations
... Count the number of atoms of each element of the __________ Add / Change the __________ to make the numbers of each element equal YOU CAN NEVER CHANGE A SUBSCRIPT! Write the coefficients in the __________ possible ratio Check your work ...
... Count the number of atoms of each element of the __________ Add / Change the __________ to make the numbers of each element equal YOU CAN NEVER CHANGE A SUBSCRIPT! Write the coefficients in the __________ possible ratio Check your work ...
SCH3U - Norbraten
... Write the word and skeletal equation for the following reactions. Be sure to include the proper states of matter by using the appropriate subscripts. You do not need to balance the equation. If the reaction does not occur write NO REACTION (NR) 10. Magnesium metal burns in air to produce solid magne ...
... Write the word and skeletal equation for the following reactions. Be sure to include the proper states of matter by using the appropriate subscripts. You do not need to balance the equation. If the reaction does not occur write NO REACTION (NR) 10. Magnesium metal burns in air to produce solid magne ...
Chemistry MSL Practical Style Review 1. What is the nuclear
... 10. What type of bonding is associated with compounds that have the following characteristics: •high melting points •conduct electricity in the molten state •solutions conduct electricity •normally crystalline solids at room temperature. A B C D ...
... 10. What type of bonding is associated with compounds that have the following characteristics: •high melting points •conduct electricity in the molten state •solutions conduct electricity •normally crystalline solids at room temperature. A B C D ...
UNIT 1 - StudyGuide.PK
... for MgSO4 + 7H2O(l) → MgSO4.7H2O(s) by dissolving each in water, and measuring the respective temperature changes; or the ΔHo for CaCO3(s) → CaO(s) + CO2(g) by dissolving each solid in HCl(aq). Numerical practice with cycles involving combustions of alkenes/alkenes; C(s), H2(g) and hydrocarbons or a ...
... for MgSO4 + 7H2O(l) → MgSO4.7H2O(s) by dissolving each in water, and measuring the respective temperature changes; or the ΔHo for CaCO3(s) → CaO(s) + CO2(g) by dissolving each solid in HCl(aq). Numerical practice with cycles involving combustions of alkenes/alkenes; C(s), H2(g) and hydrocarbons or a ...
Past AP FRQ`s Linked to Text Chapters
... - A solution of 1.0-molar HCl - A solution of concentrated HNO3 (a) Which metal can be easily identified because it is much softer than the other two? Describe a chemical test that distinguishes this metal from the other two, using only one of the reagents above. Write a balanced chemical equation f ...
... - A solution of 1.0-molar HCl - A solution of concentrated HNO3 (a) Which metal can be easily identified because it is much softer than the other two? Describe a chemical test that distinguishes this metal from the other two, using only one of the reagents above. Write a balanced chemical equation f ...
Exercise #5_Chpt 2
... Carbon tetrachloride, CCl4, can be produced in the reaction below. CH4 + 4Cl2 CCl4 + 4HCl a) What mass of CH4 is needed to exactly combine with 3.4 g Cl2? b) How many grams of Cl2 are required to produce 91 g CCl4, assuming excess CH4? c) What mass of CH4 must have reacted, if 2 mg HCl is liberate ...
... Carbon tetrachloride, CCl4, can be produced in the reaction below. CH4 + 4Cl2 CCl4 + 4HCl a) What mass of CH4 is needed to exactly combine with 3.4 g Cl2? b) How many grams of Cl2 are required to produce 91 g CCl4, assuming excess CH4? c) What mass of CH4 must have reacted, if 2 mg HCl is liberate ...
Moles Review
... (Cl), what is the empirical formula for this compound? 14) The most common form of nylon is 63.68% carbon, 12.38% nitrogen, and 14.14 % oxygen. Calculate the empirical formula. 15) The molar mass of a particular molecular compound is 180 g/mol. The percent composition of this compound is: C = 40.00% ...
... (Cl), what is the empirical formula for this compound? 14) The most common form of nylon is 63.68% carbon, 12.38% nitrogen, and 14.14 % oxygen. Calculate the empirical formula. 15) The molar mass of a particular molecular compound is 180 g/mol. The percent composition of this compound is: C = 40.00% ...
FINAL EXAM REVIEW PROBLEMS
... 45. Consider two sample of nitrogen gas. Sample 1 contains 1.5 mol of N2 and has a volume of 36.7 L at 25C and 1 atm. Sample 2 has a volume of 16.5 L at 25C and 1 atm. Calculate the number of moles of N2 in sample 2. 46. A weather balloon contains 1.10 x 103 mol of helium and has a volume of 2.70 ...
... 45. Consider two sample of nitrogen gas. Sample 1 contains 1.5 mol of N2 and has a volume of 36.7 L at 25C and 1 atm. Sample 2 has a volume of 16.5 L at 25C and 1 atm. Calculate the number of moles of N2 in sample 2. 46. A weather balloon contains 1.10 x 103 mol of helium and has a volume of 2.70 ...
Types o.. - hrsbstaff.ednet.ns.ca
... dry test tube. Set up the ring stand and secure the test tube in the test tube clamp (on a slight angle, facing away from others). Gently heat with a Bunsen burner. (1) What do you observe on the upper part of the test tube? (2) What do you observe in the bottom of the test tube? Continue to heat un ...
... dry test tube. Set up the ring stand and secure the test tube in the test tube clamp (on a slight angle, facing away from others). Gently heat with a Bunsen burner. (1) What do you observe on the upper part of the test tube? (2) What do you observe in the bottom of the test tube? Continue to heat un ...
File - chemistryattweed
... production of ammonia because two molecules of gaseous ammonia occupy a smaller volume than the four molecules of gaseous reactants. High pressure also increases the reaction rate because the gas molecules are closer and at higher concentrations. However, high-pressure equipment is expensive and r ...
... production of ammonia because two molecules of gaseous ammonia occupy a smaller volume than the four molecules of gaseous reactants. High pressure also increases the reaction rate because the gas molecules are closer and at higher concentrations. However, high-pressure equipment is expensive and r ...
KEY Midterm Exam 1 Sept.14, 1999 Chemistry 211 PAGE 1 0f 5
... The inhabitants of a planet "Htrae" in a distant galaxy measure mass in units of "margs", where 1 marg = 4.8648 grams (exactly). Their scale of atomic masses is based on the isotope 3 2S (atomic mass on earth = 31.972 g/mole), so they define one "elom" of 3 2S as the amount of sulfur atoms in exactl ...
... The inhabitants of a planet "Htrae" in a distant galaxy measure mass in units of "margs", where 1 marg = 4.8648 grams (exactly). Their scale of atomic masses is based on the isotope 3 2S (atomic mass on earth = 31.972 g/mole), so they define one "elom" of 3 2S as the amount of sulfur atoms in exactl ...
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.