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At equilibrium
... – if Q < K it follows that the reaction can only go forward. (eg. when we start with only “reactants”) – if Q > K it follows that the reaction can only go backward. (eg. When we start with only “products”) – if Q = K it follows that the reaction is at equilibrium • Therefore by finding Q at any poin ...
... – if Q < K it follows that the reaction can only go forward. (eg. when we start with only “reactants”) – if Q > K it follows that the reaction can only go backward. (eg. When we start with only “products”) – if Q = K it follows that the reaction is at equilibrium • Therefore by finding Q at any poin ...
FREE Sample Here
... Sodium iodide + lead nitrate ------> lead iodide + sodium nitrate Is this equation balanced? If not, be sure to balance it. 2 NaI + Pb(NO3)2 ------> PbI2 + 2 NaNO3 4. Place a small amount of sodium bicarbonate in a test tube and add a couple of drops of hydrochloric acid. a. What physical evidence i ...
... Sodium iodide + lead nitrate ------> lead iodide + sodium nitrate Is this equation balanced? If not, be sure to balance it. 2 NaI + Pb(NO3)2 ------> PbI2 + 2 NaNO3 4. Place a small amount of sodium bicarbonate in a test tube and add a couple of drops of hydrochloric acid. a. What physical evidence i ...
BalanceEquationsetc
... • A mole is defined as the number of atoms in exactly 12 grams of carbon- 12 • The number is called Avogadro’s Number • One mole of carbon atoms has a mass of 12 grams ...
... • A mole is defined as the number of atoms in exactly 12 grams of carbon- 12 • The number is called Avogadro’s Number • One mole of carbon atoms has a mass of 12 grams ...
CHE 1401 - Summer 2012 - Chapter 5 Homework 5 (Chapter 5
... C) ΔE = Efinal - Einitial D) Energy lost by the system must be gained by the surroundings. E) 1 cal = 4.184 J (exactly) 9) The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1°F. Th ...
... C) ΔE = Efinal - Einitial D) Energy lost by the system must be gained by the surroundings. E) 1 cal = 4.184 J (exactly) 9) The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1°F. Th ...
CHE 1401 - Fall 2015 - Chapter 5 Homework 5 (Chapter 5
... 23) What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80 oC? (The specific heat of the solution is 3.74 joules/gram-K.) A) 6.51 B) -7.43 C) 8.20 D) -9.12 E) -12.51 ...
... 23) What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80 oC? (The specific heat of the solution is 3.74 joules/gram-K.) A) 6.51 B) -7.43 C) 8.20 D) -9.12 E) -12.51 ...
Chemical Equations - Salem Community Schools
... Reactions that form water or a gas Some double-replacement reactions in aqueous solution produce water or a gas (or both) rather than a precipitate. In such cases, the water or gas is shown as a product in the net ionic equation, as are the ions that produced it. The remaining ions are eliminated as ...
... Reactions that form water or a gas Some double-replacement reactions in aqueous solution produce water or a gas (or both) rather than a precipitate. In such cases, the water or gas is shown as a product in the net ionic equation, as are the ions that produced it. The remaining ions are eliminated as ...
Chemistry Notes for the Whole Year Powerpoint
... • Even though like charges repel, the protons in the nucleus do not repel because they interact with and are spaced out by the neutrons. ...
... • Even though like charges repel, the protons in the nucleus do not repel because they interact with and are spaced out by the neutrons. ...
Honors Chemistry
... Describe the structure of the water molecule and how it determines the unique properties of water Define pressure, the units of pressure, and describe how it is measured Convert between units of pressure Use Dalton’s law of partial pressures to calculate partial and total pressures of gas mixtures U ...
... Describe the structure of the water molecule and how it determines the unique properties of water Define pressure, the units of pressure, and describe how it is measured Convert between units of pressure Use Dalton’s law of partial pressures to calculate partial and total pressures of gas mixtures U ...
Honors Chemistry Curr
... Describe the structure of the water molecule and how it determines the unique properties of water Define pressure, the units of pressure, and describe how it is measured Convert between units of pressure Use Dalton’s law of partial pressures to calculate partial and total pressures of gas mixtures U ...
... Describe the structure of the water molecule and how it determines the unique properties of water Define pressure, the units of pressure, and describe how it is measured Convert between units of pressure Use Dalton’s law of partial pressures to calculate partial and total pressures of gas mixtures U ...
Chapter 9 Stoichiometry
... How many grams of CaF2 is formed when 35.8mL of 0.678 M NaF is treated with excess of Ca(NO3)2(aq)? NaF + Ca(NO3)2 CaF2 + Na2(NO3)2 ...
... How many grams of CaF2 is formed when 35.8mL of 0.678 M NaF is treated with excess of Ca(NO3)2(aq)? NaF + Ca(NO3)2 CaF2 + Na2(NO3)2 ...
Use the following answers for questions 10
... 38. The radioactive decay of 6-C-14 to 7-N-14 occurs by the process of (A) beta particle emission (B) alpha particle emission (C) positron emission (D) electron capture (E) neutron capture 39. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the tem ...
... 38. The radioactive decay of 6-C-14 to 7-N-14 occurs by the process of (A) beta particle emission (B) alpha particle emission (C) positron emission (D) electron capture (E) neutron capture 39. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the tem ...
Chemistry 11 Exam 1 Spring 2006 When answering questions be
... 13. The atomic radii for the first four alkali metals are shown below. Explain this pattern. Moving down the periodic table the outermost occupied orbitals increase ( n= 1,2,3,4,5,...). As the outermost occupied orbital increases for n the size of the orbital also increases. For Na the outermost occ ...
... 13. The atomic radii for the first four alkali metals are shown below. Explain this pattern. Moving down the periodic table the outermost occupied orbitals increase ( n= 1,2,3,4,5,...). As the outermost occupied orbital increases for n the size of the orbital also increases. For Na the outermost occ ...
AP Stoichiometry
... 3. Divide each by the smallest number of moles to obtain the simplest whole number ratio. 4. If whole numbers are not obtained* in step 3), multiply through by the smallest number that will give all whole numbers ...
... 3. Divide each by the smallest number of moles to obtain the simplest whole number ratio. 4. If whole numbers are not obtained* in step 3), multiply through by the smallest number that will give all whole numbers ...
Chapter 15: Kinetics
... If the rate of disappearance of A is equal to -0.084 mol/L s at the start of the reaction what are the rates of change for B, C and D at this time? Rate of change of B = Rate of change of C = Rate of change of D = a) B= 0.042 M/s; C= 0.056 M/s; D= - 0.042 mol/L s b) B = -0.042M/s; C = 0.112 M/s; D = ...
... If the rate of disappearance of A is equal to -0.084 mol/L s at the start of the reaction what are the rates of change for B, C and D at this time? Rate of change of B = Rate of change of C = Rate of change of D = a) B= 0.042 M/s; C= 0.056 M/s; D= - 0.042 mol/L s b) B = -0.042M/s; C = 0.112 M/s; D = ...
2016 - Specimen Paper 4 - Cambridge International Examinations
... to show that cobalt(II) carbonate is in excess: number of moles of HCl used = ……………………….……… (use your value from above) mass of one mole of CoCO3 = 119 g number of moles of CoCO3 in 5.95 g of cobalt(II) carbonate = ………………………… [5] (ii) Explain how these calculations show that cobalt(II) carbonate is ...
... to show that cobalt(II) carbonate is in excess: number of moles of HCl used = ……………………….……… (use your value from above) mass of one mole of CoCO3 = 119 g number of moles of CoCO3 in 5.95 g of cobalt(II) carbonate = ………………………… [5] (ii) Explain how these calculations show that cobalt(II) carbonate is ...
anna-chrobok-silesian-university-of-technology
... - Diels-Alder reaction, - oxidation of alcohols and ketones. IONIC LIQUIDS as homogeneous and heterogeneous catalysts Recycling of ionic liquids prevents them from: - ending up in the aquatic environment, - release into the atmosphere (low volatility). ...
... - Diels-Alder reaction, - oxidation of alcohols and ketones. IONIC LIQUIDS as homogeneous and heterogeneous catalysts Recycling of ionic liquids prevents them from: - ending up in the aquatic environment, - release into the atmosphere (low volatility). ...
Worksheet 8 Notes - Department of Chemistry | Oregon State
... (Reduction—the oxidation number of nitrogen is decreasing from 5+ to 4+) Step 3: Balance atoms (except H and O) This step is not necessary—copper and nitrogen are balanced. Step 4: Balance oxygen by adding water This step is not necessary for the copper half-reaction. NO3- (aq) → NO2 (g) + H2O (l) S ...
... (Reduction—the oxidation number of nitrogen is decreasing from 5+ to 4+) Step 3: Balance atoms (except H and O) This step is not necessary—copper and nitrogen are balanced. Step 4: Balance oxygen by adding water This step is not necessary for the copper half-reaction. NO3- (aq) → NO2 (g) + H2O (l) S ...
Stoichiometry - hrsbstaff.ednet.ns.ca
... the molecule takes up. For example, let us take CH5N. A scientist is attempting to find the formula but doesn’t know what it is. He breaks it up and finds that 38.67% Carbon, 16.22% Hydrogen, and 45.11% Nitrogen. By assuming the compound weighs 100 grams, each of these percentages now becomes gram u ...
... the molecule takes up. For example, let us take CH5N. A scientist is attempting to find the formula but doesn’t know what it is. He breaks it up and finds that 38.67% Carbon, 16.22% Hydrogen, and 45.11% Nitrogen. By assuming the compound weighs 100 grams, each of these percentages now becomes gram u ...
WRITING AP EQUATIONS AP equation sets are found in the free
... anything about acidic or basic solution, it is redox. If you are totally stuck, look up the compounds in the index of your book or other reference books and try to find information that will help you with the equation. All reactions do not fit neatly into the five types of reactions that you learned ...
... anything about acidic or basic solution, it is redox. If you are totally stuck, look up the compounds in the index of your book or other reference books and try to find information that will help you with the equation. All reactions do not fit neatly into the five types of reactions that you learned ...
Stoichiometry
![](https://commons.wikimedia.org/wiki/Special:FilePath/Combustion_reaction_of_methane.jpg?width=300)
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.