Nitrogen and its compounds - kcpe-kcse
... The drying agent used for ammonia is quick lime. Other drying agents such as concentrated sulphuric acid or phosphorus (V) oxide or fused calcium chloride cannot dry an alkaline gas like ammonia. Sulphuric acid and phosphorus (V) oxide are both acidic. They react with ammonia, forming their respecti ...
... The drying agent used for ammonia is quick lime. Other drying agents such as concentrated sulphuric acid or phosphorus (V) oxide or fused calcium chloride cannot dry an alkaline gas like ammonia. Sulphuric acid and phosphorus (V) oxide are both acidic. They react with ammonia, forming their respecti ...
AP Chemistry Summer Assignment 2016 revised
... mole percent, 10.0% O2, 10.0% N2 , and 80.0% He. a.Calculate the molar mass of this mixture. b.What is the ratio of the density of this gas to that of pure Oxygen? 57.A 2.0g sample of SX6 (g) has a volume of 329.5 cm3 at 1.00 atm and 20oC. Identify the element ‘X’. Name the compound. 58.When Hydroge ...
... mole percent, 10.0% O2, 10.0% N2 , and 80.0% He. a.Calculate the molar mass of this mixture. b.What is the ratio of the density of this gas to that of pure Oxygen? 57.A 2.0g sample of SX6 (g) has a volume of 329.5 cm3 at 1.00 atm and 20oC. Identify the element ‘X’. Name the compound. 58.When Hydroge ...
Chemistry - Bourbon County Schools
... Calculate the percent composition of a substance, given its formula or masses of each component element in a sample ...
... Calculate the percent composition of a substance, given its formula or masses of each component element in a sample ...
Chemistry Study Guide
... position on the table will show many of its general properties Periods- The table is arranged in horizontal rows called periods. The period tells you how many electron energy levels the atom has. Groups- Vertical columns whose members of the same group have similar chemical and physical properti ...
... position on the table will show many of its general properties Periods- The table is arranged in horizontal rows called periods. The period tells you how many electron energy levels the atom has. Groups- Vertical columns whose members of the same group have similar chemical and physical properti ...
Chemistry Study Guide
... position on the table will show many of its general properties Periods- The table is arranged in horizontal rows called periods. The period tells you how many electron energy levels the atom has. Groups- Vertical columns whose members of the same group have similar chemical and physical properti ...
... position on the table will show many of its general properties Periods- The table is arranged in horizontal rows called periods. The period tells you how many electron energy levels the atom has. Groups- Vertical columns whose members of the same group have similar chemical and physical properti ...
Chemistry I Exams and Keys Corrected 2016 Season
... memorization. Also, student may not have read about Proust. All full credit. A) When two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers. B) The rate of any chemical reacti ...
... memorization. Also, student may not have read about Proust. All full credit. A) When two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers. B) The rate of any chemical reacti ...
GCSE_C2_Revision_+_Exam_Questions
... (c) Berzelius gave oxygen the number 100 to represent its relative atomic mass. He then set out to compare the mass of other elements with oxygen. However, he could not measure these directly because they could not be turned into gases – the temperature needed was too high and he did not have the eq ...
... (c) Berzelius gave oxygen the number 100 to represent its relative atomic mass. He then set out to compare the mass of other elements with oxygen. However, he could not measure these directly because they could not be turned into gases – the temperature needed was too high and he did not have the eq ...
PRE AP CHEMISTRY REVIEW PROBLEMS NON COLLEGE
... e. Aluminum metal reacts completely with chlorine gas. f. A piece of aluminum foil is dipped in a solution of cupric chloride. 36. In problem 23 for reactions a, e, f, g, h, and j, write the oxidation states of the elements and identify the element that is oxidized and the element that is reduced. 3 ...
... e. Aluminum metal reacts completely with chlorine gas. f. A piece of aluminum foil is dipped in a solution of cupric chloride. 36. In problem 23 for reactions a, e, f, g, h, and j, write the oxidation states of the elements and identify the element that is oxidized and the element that is reduced. 3 ...
Remember Question words
... Law of Conservation of Mass = no detectable gain or loss in mass occurs in chemical reactions. However, the state of a substance may change in a chemical reaction. For example, substances in a chemical reaction can change from solid states to gaseous states but the total mass will not change. Or mor ...
... Law of Conservation of Mass = no detectable gain or loss in mass occurs in chemical reactions. However, the state of a substance may change in a chemical reaction. For example, substances in a chemical reaction can change from solid states to gaseous states but the total mass will not change. Or mor ...
john dalton!! - Hawk Chemistry
... Dalton’s FOUR part atomic theory • 1) All elements are composed of tiny indivisible particles called atoms. • 2) Atoms of the same element are identical. • 3) Atoms of different elements can physically mix together or can chemically combine. • 4) Chemical reactions occur when atoms are separated, j ...
... Dalton’s FOUR part atomic theory • 1) All elements are composed of tiny indivisible particles called atoms. • 2) Atoms of the same element are identical. • 3) Atoms of different elements can physically mix together or can chemically combine. • 4) Chemical reactions occur when atoms are separated, j ...
Spring 2002 - Kwantlen Polytechnic University
... b. The solution shows a positive deviation from Raoult’s Law. c. The solution shows a negative deviation from Raoult’s Law and possesses a minimum boiling point azeotrope. d. The solution shows a negative deviation from Raoult’s Law and possesses a maximum boiling point azeorope. e. The solution pro ...
... b. The solution shows a positive deviation from Raoult’s Law. c. The solution shows a negative deviation from Raoult’s Law and possesses a minimum boiling point azeotrope. d. The solution shows a negative deviation from Raoult’s Law and possesses a maximum boiling point azeorope. e. The solution pro ...
50 Forgotten Facts
... 28) ONLY metals with more than one listed charge need a Roman numeral after their name (Stock system) when naming an ionic compound. Nonmetals with more than one oxidation state will also need a Roman numeral in their name if they are the less electronegative atom in a molecular compound. [P. T., Ta ...
... 28) ONLY metals with more than one listed charge need a Roman numeral after their name (Stock system) when naming an ionic compound. Nonmetals with more than one oxidation state will also need a Roman numeral in their name if they are the less electronegative atom in a molecular compound. [P. T., Ta ...
Chemical Reactions: Helpful Hints
... Reaction 8 involves a base and an ammonium salt. (The tricky part here is to explain why the gas reacted with the wet pH paper and not the dry pH paper the gas reacted with the water on the pH paper to generate a base, hence the pH paper turned blue - I've given you the reactants, you should be ab ...
... Reaction 8 involves a base and an ammonium salt. (The tricky part here is to explain why the gas reacted with the wet pH paper and not the dry pH paper the gas reacted with the water on the pH paper to generate a base, hence the pH paper turned blue - I've given you the reactants, you should be ab ...
PPT format - Columbia University
... Section 1.2 The Composition of Matter and Section 1.3: The Atomic Theory of Matter. Matter: Matter is any material that occupies space and has mass. Atomic interpretation: Any material that contains atoms, which occupy space and have mass. Substance (idealization): A substance is a chemically pure ...
... Section 1.2 The Composition of Matter and Section 1.3: The Atomic Theory of Matter. Matter: Matter is any material that occupies space and has mass. Atomic interpretation: Any material that contains atoms, which occupy space and have mass. Substance (idealization): A substance is a chemically pure ...
Chapter 5: thermochemstry
... More on hess’ law • Hess' law allows ΔH rxn to be calculated even when it can’t be measured directly. • To do this, we perform arithmetic operations on chemical equations and known ΔH values. – Chemical equations may be multiplied or divided by a whole number. – When an equation is multiplied by a c ...
... More on hess’ law • Hess' law allows ΔH rxn to be calculated even when it can’t be measured directly. • To do this, we perform arithmetic operations on chemical equations and known ΔH values. – Chemical equations may be multiplied or divided by a whole number. – When an equation is multiplied by a c ...
AP Chemistry Summer Assignment
... 59. An open flask contains 0.200 mol of air. Atmospheric pressure is 745 mmHg and room temperature is 68˚F. How many moles are present in the flask when the pressure is 1.10 atm and the temperature is 33˚C? 60. On a warm day, an amusement park balloon is filled with 47.8 g He. The temperature is 33˚ ...
... 59. An open flask contains 0.200 mol of air. Atmospheric pressure is 745 mmHg and room temperature is 68˚F. How many moles are present in the flask when the pressure is 1.10 atm and the temperature is 33˚C? 60. On a warm day, an amusement park balloon is filled with 47.8 g He. The temperature is 33˚ ...
10th Grade Chemistry X (TJ) GRADE(S)/LEVELS SUBJECT Power
... Use stoichiometry to predict quantities in chemical reactions. LT 1 Use a balanced equation to predict the quantities of reactants and products that are required or produced in a chemical reaction. LT 2 Identify the limiting reagent and determine the theoretical yield of a reaction. LT 3 Calculate t ...
... Use stoichiometry to predict quantities in chemical reactions. LT 1 Use a balanced equation to predict the quantities of reactants and products that are required or produced in a chemical reaction. LT 2 Identify the limiting reagent and determine the theoretical yield of a reaction. LT 3 Calculate t ...
Chem Regents 2015 A Few Things
... Strong acids: hydrochloric acid HCl, nitric acid HNO3, sulfuric acid H2SO4 Weak acids: carbonic acid H2CO3, acetic acidCH3COOH ...
... Strong acids: hydrochloric acid HCl, nitric acid HNO3, sulfuric acid H2SO4 Weak acids: carbonic acid H2CO3, acetic acidCH3COOH ...
Name ionic compounds containing main group or
... How many moles are there in 3.67 x 1024 atoms of helium gas? Helium (He) is #2. I am holding 0.0452 moles of a pure element and it weighs 542 mg. What element is it? How much would 7.12 109 formula units of silver sulfate weigh in grams? The formula mass of silver sulfate is 312 g/mole If 499.5 gr ...
... How many moles are there in 3.67 x 1024 atoms of helium gas? Helium (He) is #2. I am holding 0.0452 moles of a pure element and it weighs 542 mg. What element is it? How much would 7.12 109 formula units of silver sulfate weigh in grams? The formula mass of silver sulfate is 312 g/mole If 499.5 gr ...
Calculation Booklet - Clydebank High School
... Radioactivity and Halflife Half-life is the time taken for half of a radioisotope to decay. This value is constant for that particular isotope. ...
... Radioactivity and Halflife Half-life is the time taken for half of a radioisotope to decay. This value is constant for that particular isotope. ...
Thermochemistry
... Recall: All chemical reactions either release (exothermic) or absorb (endothermic) heat energy when going from reactants → products. As we saw in earlier material, this information can be represented quantitatively with a thermochemical equation. Example: CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) ; Δ ...
... Recall: All chemical reactions either release (exothermic) or absorb (endothermic) heat energy when going from reactants → products. As we saw in earlier material, this information can be represented quantitatively with a thermochemical equation. Example: CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) ; Δ ...
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.