Answer All These Questions, Must Be Submitted In 2

Answer All Of Theses Questions And It Must Be Submitted In 2 Hours Ple

Answer all of theses questions and it must be submitted in 2 hours please be on time Question 1 (2 points) What is the density of a block of unknown material with a mass of 11.90-g if the dimensions are: length = 2.2 cm height = 1.7 cm width = 7.5 cm Question 2 (2 points) What is the density of a 16.97-g object if the dimensions of the block are: length = 12.6 mm height = 6.8 cm width = 0.014 m Question 3 (2 points) What is the density of a 21.73-g irregularly shaped object if the initial volume of water was 23.4-mL and the volume rose to 56.0-mL after the object was added? Question 4 (2 points) A volume of water was delivered using a buret and experimentally determined to have a mass of 2.44-g. What was the final volume of water on the buret if the initial was 0.17-mL? [assume the density of water is 1.00g/mL] Question 5 (2 points) Identify the following chemical using the information provided below: initial buret reading: 1.2-mL final buret reading: 10.5-mL mass: 8.184-g ------ Question 1 (2 points) What is the name of N2O5? Question 2 (2 points) What is the name of the compound composed of Ca and P? Question 3 (2 points) What is the formula for the compound composed of calcium and phosphate? Question 4 (2 points) What is the name of the compound composed of iron and carbonate? [Hint: iron has a +3 charge in this compound] Question 5 (2 points) Match the following acids to the correct names: sulfuric acid hydrosulfuric acid sulfurous acid H2SO4 H2SO3 H2S ---- Question 1 (2 points) Cu+2 forms which color when dissolved in water? Question 2 (2 points) Calculate the percent recovery of copper if: 1.5-g is the initial amount and 1.2-g is the amount recovered. [Hint: do not include the percentage sign when typing in your answer] Question 3 (2 points) Which of the following is NOT a good explination/indication as to the results obtained in the above question? Question 4 (2 points) Calculate the percent recovery of copper if: 7.6-g is the initial amount and 9.5-g is the amount recovered. [Hint: do not include the percentage sign when typing in your answer] Question 5 (2 points) Which of the following is NOT a good explination/indication as to the results obtained in the above question? ---- Question 1 (2 points) Once acid was added to the supplement, what was the purpose of filtering the solution? Save Question 2 (2 points) When sodium carbonate is added to the filtrate, fizzing occurs. Which gas is being produced? Question 3 (2 points) What was the purpose of heating the calcium carbonate precipitate? Question 4 (2 points) How many milligrams of calcium is in 1.46-g of calcium carbonate? Question 5 (2 points) What is the percent mass of calcium in a calcium supplement if 1.34-g of calcium carbonate is extracted from a 2.80-g pill? ----- Quiz Question 1 (2 points) How much heat is lost by 5 grams of a metal if the temperature changed from 90c to 40c? (c=3.95 J/gK) Save Question 2 (2 points) Assume a piece of hot metal is added to a colorimeter containing 50mL of water at 22C. The amount of heat released by the metal was determined to be 1000 J, and the equilibrium temperature in the calorimeter was 26C. Remembering that the specific heat of water is 4.18 J/gC, how much heat in joiles does the clorimeter gain? Save Question 3 (2 points) Assume the heat absorbed by the calorimeter was 200 J. What is the calorimeter constant (Heat Capacity) if the temperature changed from 22C to 26C? Save Question 4 (1 point) Calculate the Calorimeter Constant if 25 g of water at 58C was added to 25 g of water at 25C with a resulting temperature of 35C? Save ------ Question 1 (2 points) What is the definition of the Enthalpy of Reaction? Save Question 2 (2 points) Which of the following reactions needs to be reversed to solve for the Heat of Neutralization between Hydrochloric Acid and Ammonia? Save Question 3 (2 points) What is the molar heat of neutralization (Enthalpy of Reaction) in kJ/mol if 5 moles of HA neutralized 5 moles of BOH and released 11123 J of heat? Save Question 4 (2 points) Calculate the molar heat of neutralization in kJ/mol of the reaction between HA and BOH given the following information: The temperature change equals 5C, 50 mL of 1 M concentration of Acid 50 mL of 1 M concentration of Base Heat capacity of the calorimeter is 6.5 J/C. Remember that the specific heat of water is 4.18 J/gC Save Question 5 (2 points) How much heat is gained (in Joules) by the water where a chemical reaction takes place in 100 mL aqueous solution and has a temperature increase of 12 C? Save ---- Question 1 (2 points) What is the definition of the Enthalpy of Reaction? Save Question 2 (2 points) Which of the following reactions needs to be reversed to solve for the Heat of Neutralization between Hydrochloric Acid and Ammonia? Save Question 3 (2 points) What is the molar heat of neutralization (Enthalpy of Reaction) in kJ/mol if 5 moles of HA neutralized 5 moles of BOH and released 11123 J of heat? Save Question 4 (2 points) Calculate the molar heat of neutralization in kJ/mol of the reaction between HA and BOH given the following information: The temperature change equals 5C, 50 mL of 1 M concentration of Acid 50 mL of 1 M concentration of Base Heat capacity of the calorimeter is 6.5 J/C. Remember that the specific heat of water is 4.18 J/gC Save Question 5 (2 points) How much heat is gained (in Joules) by the water where a chemical reaction takes place in 100 mL aqueous solution and has a temperature increase of 12 C? Save ---- Question 1 (2 points) What is the wavelength of light (in nm) if the frequency is 6.2 x 10^14 (1/sec)? Save Question 2 (2 points) What is the wavelength of light (in nm) if the energy of the wave is 1.87 x 10^-19 J? Save Question 3 (2 points) What is the final concentration of a solution if 106-mL of a 3.3-M solution was diluted to 487-mL? Save Question 4 (2 points) What is the final concentration of a solution if 15-mL of a 2.0-M solution was diluted to 100-mL and this process was repeated two more times? Save Question 5 (2 points) Using the attached chart, find the concentration of a solution if the absorption was 0.27. Save ---- Question 1 (2 points) How many lone pairs of electrons are there on the central atom in ammonia (NH3)? Save Question 2 (2 points) What is the electronic geometry of PCl5? Save Question 3 (2 points) What is the molecular geometry of NH3? Save Question 4 (2 points) What is the orbital hybridization of the central atom S in SF4? Save Question 5 (2 points) Is S=C=O a polar molecule? ----- A sample of gas occupies 27 L under a pressure of 1.3 atm. What would the resulting volume be if the pressure were increased to 3.9 atm if the temperature did not change? ----- A sample of CO2 occupies 200 ml at 373 K. At what temperature (in K) would it occupy 300 ml if the pressure did not change? ------- A sample of Helium occupies 200 L at 30ºC under a pressure of 855 torr. What is the volume it occupies at standard temperature and pressure (STP)? ------- Nitric acid, a very important industrial chemical, is made by dissolving the gas nitrogen dioxide (NO2) in water. Calculate the moles of gas produced in 2 L volume container, 762 torr and 50 ºC if the gas behaves as ideal: ------- An unknown amount of sodium bicarbonate reacts with excess hydrochloric acid in a gas producing reaction. The reaction vessel has the same set-up as that in lab. Paying attention to the partial pressures of water in your lab book, if 119-mL of salt water was collected in the beaker at 23C and 765mmHg, how many grams of sodium bicarbonate did one begin with? -- Should be submitted in less than two hours

Paper For Above instruction

The collection of questions presented encompasses various fundamental principles in chemistry including density calculations, molar conversions, gas law computations, solution concentrations, and reaction energetics. This comprehensive overview entails precise mathematical calculations and conceptual understanding of physical and chemical properties to accurately address each problem within the stipulated constraints and deadline constraints.

Introduction

Chemistry involves understanding the properties of matter and energy transfer. The questions focus on core topics such as density, molarity, gas laws, reaction enthalpy, and solution chemistry. These core principles are essential in both academic and practical chemistry applications, underpinning processes like material characterization, solution preparation, thermodynamics, and industrial chemical synthesis.

Density Calculations

To begin, the density of a substance is calculated using the formula: Density = Mass / Volume. For question 1, the volume of the unknown material is derived from its dimensions: volume = length × width × height. Substituting the given values, volume = 2.2 cm × 1.7 cm × 7.5 cm = 28.05 cm³. The density then is 11.90 g / 28.05 cm³ ≈ 0.424 g/cm³.

Question 2 involves initial measurements in different units, necessitating conversion to a consistent unit system, typically cubic meters or centimeters. Length = 12.6 mm = 0.0126 meters, height = 6.8 cm = 0.068 meters, width = 0.014 meters. The volume in cubic meters is 0.0126 m × 0.068 m × 0.014 m = 1.19 × 10^-5 m³. The mass is 16.97 g = 0.01697 kg, so density = 0.01697 kg / 1.19 × 10^-5 m³ ≈ 1427.73 kg/m³.

Density from Displacement Method

Question 3 applies Archimedes’ principle, where the volume of the irregular object is equal to the volume of water displaced. The volume displaced is ΔV = 56.0 mL - 23.4 mL = 32.6 mL. The density of the object is mass/volume: 21.73 g / 32.6 mL ≈ 0.667 g/mL.

Solution Volumes

Question 4 involves calculating the final volume based on water mass and density. Since the mass of water is 2.44 g and the density is 1.00 g/mL, the volume is 2.44 mL. If initial volume was 0.17 mL, then the total volume after addition is 0.17 mL + 2.44 mL = 2.61 mL.

Chemical Identification from Titration Data

Question 5 requires deducing the chemical identity from titration data and mass. The titration involves the volume of titrant used—(final buret reading – initial = 10.5 mL – 1.2 mL = 9.3 mL). With the mass of 8.184 g, further information about titrant molarity is needed for precise identification; however, typical acids or bases in titrations include acids such as HCl, H2SO4, or bases like NaOH.

Material and Solution Analysis

The questions concerning chemical compounds involve recognizing chemical names and formulas based on constituent elements and oxidation states. N2O5 is dinitrogen pentoxide, a nitrogen oxoacid anhydride. Compounds with Ca and P likely refer to calcium phosphates such as hydroxyapatite (Ca10(PO4)6(OH)2) formulated as Ca3(PO4)2. Iron carbonate with Fe³⁺ is Fe2(CO3)3. Correspondingly, acids are matched: sulfuric acid (H2SO4), sulfurous acid (H2SO3), hydrosulfuric acid (H2S).

Transition Metal and Complex Chemistry

Copper(II) ions generally impart a blue or green color when dissolved in water owing to d-d electronic transitions. Percent recovery calculations assess the effectiveness of extraction procedures in chemical reactions. For example, initial copper mass is 1.5 g, recovered 1.2 g; percent recovery = (1.2 / 1.5) × 100 = 80%. Anomalously high recovery (e.g., exceeding initial mass) indicates experimental error or contamination.

Reactions, Acid-Base, and Thermodynamics

The purpose of filtering solutions after adding acid is to remove insoluble impurities or precipitates. When sodium carbonate is added to the filtrate and fizzing occurs, CO₂ gas is produced. Heating calcium carbonate drives off CO₂ and converts it to calcium oxide. The mass of calcium in calcium carbonate can be computed via molar ratios and molar mass calculations; for 1.46 g of calcium carbonate, the calcium content is (40.08 g/mol Ca / 100.09 g/mol CaCO3) × 1.46 g ≈ 0.586 g.

Heat and Calorimetry

Calculating the heat lost or gained involves the formula Q = mcΔT, where m is mass, c is specific heat capacity, and ΔT is temperature change. For example, 5 g of a metal with c = 3.95 J/g·K changing from 90°C to 40°C results in heat loss of Q = 5 g × 3.95 J/g·K × (90°C - 40°C) = 987.5 J.

When a hot metal transfers heat to water, calorimetry allows calculation of heat exchanged and calorimeter constants. The heat gained by water can be calculated with Q = mcΔT, and the heat released by the metal is used to determine the calorimeter’s heat capacity.

Thermochemistry and Reaction Enthalpy

The enthalpy of reaction (ΔH) is defined as the heat absorbed or released during a chemical reaction at constant pressure. To find molar enthalpy, the total heat is divided by moles of reactant. For neutralization reactions, the ΔH typically has negative values indicating exothermicity, calculated from experimental heat and moles involved.

Physics of Light and Solutions

The wavelength (λ) of light is related to its frequency (ν) via λ = c / ν, where c is the speed of light (3.0 × 10⁸ m/s). For question 1, λ = (3.0 × 10⁸ m/s) / (6.2 × 10¹⁴ 1/sec) ≈ 4.84 × 10^-7 m = 484 nm. For energy-based calculations, λ = hc / E, with Planck’s constant h = 6.626 × 10^-34 Js.

Dilution calculations follow the formula C₁V₁ = C₂V₂. For a 3.3 M solution diluted from 106 mL to 487 mL, C₂ = (3.3 M × 106 mL) / 487 mL ≈ 0.72 M. Repeated dilution further reduces concentration accordingly.

Electronic and Molecular Geometry

Ammonia (NH₃) has 1 lone pair on nitrogen and 3 bonding pairs, giving a tetrahedral electron geometry, with a trigonal pyramidal molecular geometry. PCl₅ exhibits a trigonal bipyramidal electron grammar. SF₄ exhibits a seesaw shape, and S in SF₄ hybridizes as sp³d.

Polarity and Gas Laws

S=C=O has a linear structure with polar bonds; it is a polar molecule. Using the ideal gas law PV = nRT, a gas occupying 27 L at 1.3 atm, at a higher pressure of 3.9 atm (at constant temperature), would have a volume V₂ = V₁ × (P₁ / P₂) = 27 L × (1.3 atm / 3.9 atm) ≈ 9 L. For temperature effects, P₁V