Inorganic Chemistry Questions

When aluminum, Al, metal is dipped in an aqueous solution of hydrochloric acid, HCl, hydrogen gas, H₂, is produced with the formation of an aluminum chloride, AICI3, solution Write the balanced chemical equation showing the phases of reactants and products

A sample of neon gas occupies a volume of 6.40 L at 69.0°C and 400. torr. If the volume of the gas sample is increased to 8.99 L, while its temperature is decreased to 3.0°C, the resulting gas pressure will be torr.

Magnesium metal can be dissolved by hydrochloric acid in order to produce hydrogen gas according to the following reaction: 2 HCl(aq) + Mg(s) → MgCl₂ (aq) + H₂(g) A 39.9 gram block of magnesium metal is placed into a beaker containing 2.50 L of 0.60 M hydrochloric acid. Determine the theoretical yield (in grams) of hydrogen gas. [Hint: this is a limiting reactant problem.]

Selective serotonin reuptake inhibitors (SSRIs) are commonly prescribed antidepressants. SSRIs block the reabsorption of the neurotransmitter serotonin in the brain. Changing the balance of serotonin helps brain cells send and receive chemical messages, which in turn boosts mood. Two SSRI medications are Cipralex (escitalopram, C20 H21 FN2O) and Zoloft (sertraline, C17H17 Cl₂N). Determine the molar masses of Cipralex and Zoloft. Molar mass of Cipralex = Molar mass of Zoloft =

In a coffee cup calorimetry experiment, 28.6 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 MHCI. The temperature of the solution increased by 61.3 °C. Calculate AH, in kJ/mole, for the reaction. Use 1.00 g/ mL as the density of the solution and 4.18 J/g °C as the specific heat capacity. Provide answer to 3 significant figures and do not include the unit. Do not use scientific notation.

Hybrid Orbitals Hybrid orbitals are formed by combining the valence orbitals on an atom. A molecule has sp³ hybridization with 2 lone pairs. The electron pair geometry of this molecule is: The geometry of this molecule is: This molecule will have an approximate bond angle of (If more than one bond angle is possible, separate each with a space.

With a partner or a small group, share ideas about the following topics. Then have each person write a paragraph about one of the topics. 1. What are some changes that a fast-food restaurant might have to make when it opens a franchise in another country? Consider, for example, the food, the people, and the local customs. 2. Why are small, independent retail businesses inclined to disappear when franchise stores open nearby? 3. Many companies are now creating franchises in developing countries. Do you think these franchises help or hurt the economies of these countries? Explain your opinion.

Acetylene gas, C₂H₂, used in welders' torches, releases 1300 kJ of heat when 1 mole of C₂H₂ undergoes combustion. Write a balanced equation for the reaction.

A chemistry student needs 55.0 mL of pentane for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of pentane is 0.626 g cm³. Calculate the mass of pentane the student should weigh out. Round your answer to 3 significant digits.

Suppose a group of volunteers is planning to build a park near a local lake. The lake is known to contain low levels of arsenic (As). Therefore, prior to starting construction, the group decides to measure the current level of arsenic in the lake. If a 14.9 cm³ sample of lake water is found to have 164.5 ng As, what is the concentration of arsenic in the sample in parts per billion (ppb), assuming that the density of the lake water is 1.00 g/cm³?

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H₂SO4 solution is required to neutralize a 25.0 ml sample of the NaOH solution? Select one: a. 0.801 b. 0.629 c. 125 d. 0.400 e. 0.315

No' and Ag' differ in Na2,CO3, is thermally stable while Ag,CO, decomposes into Ag2,O, CO2, and 02, Ag' forms complexes, Na' does not NaCl is water soluble, AgCl is insoluble NaCl and AgCl both give colour in flame when ignited

Iron metal can be produced by reducing iron(III) oxide with hydrogen as follows: Fe2O3(s) + 3 H₂(g) -> 2 Fe(s) + 3 H2O(g) Answer the following questions if the AH = +98.8 kJ and AS° = +141.5 J/K for the above reaction. (i) Is this reaction spontaneous under standard-state conditions (25 °C)? (Clue: Use the free energy expression, (ii) At what temperature the reaction can get the equilibrium condition?

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C. 7.94 kg 1.26 kg 1.51 kg 3.64 kg 6.62 kg

A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ---M. 1.48 6.75 2.70 0.270 0.675

Which of the following is NOT true? The Bronsted-Lowry Model applies to a wider range of acid-base phenomena than does the Arrhenius Model. The Arrhenius Model of acids and bases was developed before the Bronsted-Lowry Model. The Bronsted-Lowry Model can apply to bases that do not contain hydroxide ions. The Arrhenius Model of acids and bases applies toward substances that are nonaqueous.

What will be the molecular geometry of an open-chain noncyclical hydrocarbon with the generic molecular formula CnH2n-2? Tetrahedral Linear Trigonal planar Octahedral trigonal pyramidal

Which of the compounds of H₂C2O4, Ca(OH)2, KOH, and HI, behave as acids when they are dissolved in water? only HI H₂C2O4 and HI Ca(OH)2 and KOH only H₂C2O4 only KOH

A 12.8 g sample of ethanol (C₂H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/°C. Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C. The molar mass of ethanol is 46.07 g/mol. C₂H5OH(l) + 3 O2(g) → 2 CO₂(g) + 3 H₂O(g) ΔH°rxn = -1235 kJ 85.7°C 53.4°C 74.2°C 111°C 28.1°C

A compound is found to be 30.45% N and 69.55 % by mass. If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the molecular formula of the compound? N4O₂ NO₂ N₂O5 N₂O N₂O4

Two compounds are considered as isomers if they have the: different molecular formula AND same structure. same molecular formula AND different structure. different molecular formula AND different structure. same molecular formula AND same structure. same molecular formula OR same structure.

How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below? Assume that there is excess Fe₂O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn= -852 kJ 51.2 kJ 448 kJ 1617 kJ 808 kJ 224 kJ

Determine the theoretical yield and the percent yield if 21.8 g of K₂CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP). The molar mass of KO2 = 71.10 g/mol and K₂CO3 = 138.21 g/mol. 4 KO2(s) + 2 CO2(g) → 2 K₂CO3(s) + 3 O2(g) 61.0 g. 35.7% yield 179 g. 12.2 % yield 91.7 g. 23.8 % yield 206 g. 10.6 % yield 27.1 g, 80.4 % yield

Given three cylinders containing O₂ gas at the same volume and pressure. Cylinder A is at -15°C, cylinder B is at -5°F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen? cylinder A cylinder B cylinder C All cylinders contain the same mass of O₂.

In the following reaction: HCO3(aq) + H₂(aq) → H₂CO3 (aq) + OH (aq) Which of the following statement is true? HCO3 is an acid and H₂CO3 is its conjugate base. H₂O is an acid and HCO3 is its conjugate base. H₂o is an acid and OH is its conjugate base. HCO3 is an acid and OH is its conjugate base. H₂O is an acid and H₂CO3 is its conjugate base.

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains C₂H4, flask B contains O3, and flask C contains F2. Which flask contains the largest number of molecules? flask B flask A flask C All contain same number of molecules.

A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K? 10.2 atm 15.3 atm 1.05 atm 9.83 atm 6.53 atm

Choose the statement below that is TRUE. The term "weak electrolyte" means that the substance is inert. A molecular compound that does not ionize in solution is considered a strong electrolyte. A weak acid solution consists of mostly nonionized acid molecules. A strong acid solution consists of only partially ionized acid molecules. The term "strong electrolyte" means that the substance is extremely reactive.

Calculate the concentration of H3O* in a solution that contains 5.5 x 10-5 M OH at 25°C. Identify the solution as acidic, basic, or neutral. 1.8 x 10^-10 M, basic 9.2 x 10^-1 M, acidic 9.2 x 10^-1 M, basic 5.5 x 10^-10 M, neutral 1.8 x 10^-10 M, acidic

Using periodic trends, arrange the following atoms in order of decreasing electronegativity: Highest Lowest Si > Ga>Sr> Cl Cl> Si > Ga> Sr Si > Cl> Ga> Sr Sr> Ga> Si > Cl Sr> Ga> Cl> Si

Which statement about boiling point is FALSE? The boiling point is higher for compounds with strong intermolecular forces. The boiling point of a compound is higher for nonvolatile compounds. The boiling point of a compound is an absolute constant. The boiling point is higher for compounds with a high viscosity.

What conditions trigger the release of ADH and what is ADH's mechanism of action? What conditions trigger the release of aldosterone and what is aldosterone's mechanism of action? Describe how the body compensate in a state of respiratory acidosis?

A coffee cup calorimeter is used to study a reaction. The temperature of the water/solution drops as the reaction takes place. • Is the reaction endothermic or exothermic? . Will qsoln be positive or negative? • Will ΔHrxn be positive or negative?

Watch this short video demonstration of the alkali metals reacting with water. Each of the metals react with water in the same way, shown here for sodium: 2 Na (s) + 2 H₂O (l) ---> H₂ (g) + 2 NaOH(aq) Explain what you observe in the video using your knowledge of electronic structure and periodic properties.

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K₂O(s) + 2 N₂(g) + 5O₂(g) 1.73 mol 0.580 mol 18.5 mol 0.290 mol 0.724 mol

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O₂(g) → 3 CO2(g) + SO2(g) + 4H₂O(g) 4.14 moles 2.33 moles 1.55 moles 6.21 moles 3.50 moles

Which of the following statements about crystalline and amorphous solids is TRUE? An example of an amorphous solid is table salt (NaCl). An example of a crystalline solid is glass. A crystalline solid is composed of atoms or molecules arranged with long-range repeating order. An amorphous solid is composed of atoms or molecules with a majority of its volume empty.

What is the hydronium ion concentration of a 0.200 M acetic acid solution with Ka = 1.8 x 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H₂O(I) =H3O+ (aq) + CH3CO2−(aq). 1.9 × 10-3 M 4.2 x 10-2 M 1.9 × 10-2 M 4.2 × 10-3 M

The solubility of Pb(NO3)2 is 55 grams per 100 g H₂O at 20°C. Which term would properly describe a solution where 44 grams of Pb(NO3)2 is added to 100 grams of water at this temperature? unsaturated supersaturated insoluble saturated

If the solubility of sodium acetate (Molar mass = 82 g/mol) is 76 grams per 100 grams of water, which of the following solutions would be considered supersaturated? 1.2 moles of sodium acetate dissolved in 200 mL of water 8.5 moles of sodium acetate dissolved in 1 L of water 5.5 moles of sodium acetate dissolved in 500 mL of water 1.8 moles of sodium acetate dissolved in 300 mL of water

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) | Mg2+ (aq, 2.74 M) Pb2+ (aq, 0.33 M) | Pb(s) Mg2+ (aq) + 2e → Mg(s) E° = -2.37 V E° = -0.13V Pb2+ (aq) + 2e → Pb(s) +2.71 V +2.21 V -1.94 V -2.80 V +2.62 V

Exactly 17.0 mL of a H₂SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH. What was the concentration of the H₂SO4 solution? Given: H₂SO4 (aq) + 2NaOH (aq) → 2H₂O(l) + Na₂SO4 (aq) 0.311 M 0.622 M 0.269 M 5.63 M 0.00529 M

For the galvanic cell reaction, expressed below using shorthand notation, what half- reaction occurs at the cathode? Zn(s) | Zn2+ (aq) | Cu2+ (aq) | Cu(s) Zn2+ (aq) + 2 e → Zn(s) Zn(s) → Zn2+ (aq) + 2 e¯ Cu(s) → Cu2+ (aq) + 2 e¯ Cu2+ (aq) + 2e → Cu(s)

A solution contains 100.0 g water, 10.0 g NaCl, and 15.0 g methanol. What is the mass percent of methanol in the solution? 25% 8.00% 10.0% 12.0% 15.0%

In the following reaction, Mg (s) + Cu2+ (aq) → Mg2+(aq) + Cu (s): A) Mg is the reducing agent and Cu is the oxidizing agent. B) Mg2+ is the reducing agent and Cu is the oxidizing agent. C) Cu is the reducing agent and Mg2+ is the oxidizing agent. D) Cu2+ is the reducing agent and Mg is the oxidizing agent. E) Mg is the reducing agent and Cu2+ is the oxidizing agent. D C A E B

Radioactive isotopes with high atomic numbers often decay to form isotopes that are themselves radioactive, and once formed, decay to form new isotopes. Sometimes a series of such decays occurs over many steps until a stable nucleus is formed. The following series of decays occurs: Polonium-218 decays with emission of an a particle to form X, which emits a ß particle to form Y, which emits an particle to form Z. Identify X, Y, and Z. Give all nuclei in the form AZX. X: Y: Z:

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3 Cl2(g) + 2 Fe(s) →6 CI (aq) + 2 Fe³+ (aq) Cl2(g) + 2 e 2 E° = +1.36 V Cl(aq) Fe³+ (aq) + 3 e¯ → E° = -0.04 V Fe(s) +1.40 V -1.32 V -1.40 V +4.16 V +1.32 V

Which one of the following processes produces a decrease in the entropy of the system? melting solid aluminum into liquid aluminum deposition of solid CO2 from gaseous CO2 dissolution of LiOH(s) in water mixing of two gases into one container evaporation of liquid hexane into gaseous hexane

Which statement about surface tension is FALSE? Items with densities lower than water will sink due to surface tension. Increased intermolecular forces increase surface tension. Liquids tend to minimize their surface area. Molecules on the surface of the liquid have fewer molecules to interact wit

Here is the discussion forum for chapter 12. In addition to posting an answer the question asked, you are to explain your answer. After posting your response, I was two responses submitted by fellow students. You must make your post before you will be allowed to post your comments. Why are there no base pairs in DNA between adenine and guanine or thymine and cytosine?