Inorganic Chemistry Questions

For the following reaction, 56.3 grams of barium hydroxide are allowed to react with 30.3 grams of sulfuric acid. barium hydroxide (aq) + sulfuric acid(aq) --> barium sulfate(s) + water(l) What is the maximum amount of barium sulfate that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?

Which of the following are conclusions from Rutherford's Gold Foil Experiment? Select all that apply. Most of the atom's volume is occupied by nearly zero-mass particles. The nucleus is negatively charged. The atom's mass is uniformly distributed throughout its volume. Essentially all of the mass is concentrated in a tiny spot. Neutral (no charge) particles are found throughout the atom's volume.

The compound sodium thiosulfate pentahydrate, Na2S2O3-5H₂O, is important commercially to the photography business as "hypo", because it has the ability to dissolve unreacted silver salts from photographic film during development. Sodium thiosulfate pentahydrate can be produced by boiling elemental sulfur in an aqueous solution of sodium sulfite. S8 (s) + Na₂SO3(aq) + H₂O(l) → Na2S2O3.5H₂O(s) (unbalanced) What is the theoretical yield of sodium thiosulfate pentahydrate when 2.90 g of sulfur is boiled with 14.4 g of sodium sulfite? Theoretical yield = Sodium thiosulfate pentahydrate is very soluble in water. What is the percent yield of the synthesis if a student doing this experiment is able to isolate (collect) only 5.20 g of the product? Percent yield =

Isotopes differ in the number of _ inside the nucleus and therefore they differ in _. Select the choice that correctly fills in the blanks protons, charge protons, mass electrons, charge electrons, mass neutrons, mass

What is the change in internal energy of the system? Express the internal energy in kilojoules to three significant figures.

What is the enthalpy for reaction 1 reversed? reaction 1 reversed: 2NO+ O2---> 2NO2

Determine the enthalpy for this reaction: 2NaOH(s) + CO₂ (g)→Na2CO3 (s) + H₂O(l)

The molar heat capacity of silver is 25.35 J/mol · °C. How much energy would it take to raise the temperature of 9.90 g of silver by 15.3 °C?

Calculate ΔE, if a system releases 66.4 kJ of heat to its surroundings while the surroundings do 41.0 kJ of work on the system. Express your answer in kilojoules using two significant figures.

Match the following solution with the condition identified (name precipitate for 1 extra bonus point each if there is one. If you put wrong precipitate, there is a minus one point) a. (Answer_) K2SO4 & Na2CO3 b. (Answer_) BaCl2 & KOH (PPT) Solid will form, Precipitation (NX) No Precipitation, No Reaction

It takes 54.0 J to raise the temperature of an 9.90 g piece of unknown metal from 13.0°C to 24.9 °C. What is the specific heat for the metal? Express your answer with the appropriate units.

The amount of boiling water required to raise the temperature of 25.0 kg of water in the bath to body temperature is 4.80 kg. In this process, the heat lost by the boiling water is equal to the heat gained by the room-temperature water. How much heat was transferred in this process? Express your answer to four significant figures and include the appropriate units.

Identify whether each process is endothermic or exothermic: 1. the process from Part A: q = 0.768 kJ and w = -890 J ; 2. the process from Part B: a system releases 66.4 kJ of heat to its surroundings while the surroundings do 41.0 kJ of work on the system. Both the processes from Parts A and B are endothermic. The process from Part A is endothermic and the process from Part B is exothermic. Both the processes from Parts A and B are exothermic. The process from Part A is exothermic and the process from Part B is endothermic.

Propane (C3H8) burns according to the following balanced equation: C3H8(g) +5O2(g) →3CO₂(g) + 4H₂O(g) Calculate ΔH for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/mol.) Express the enthalpy in kilojoules to four significant figures.

Calculate the enthalpy change for the reaction: using enthalpies of formation: 2 H₂O₂(l)→ 2 H₂O(l) + O₂(g) ΔH° ƒ [H₂O2] = −187.8 kJ/mol ΔH° ƒ [H₂O] = -285.8 kJ/mol -98.0 kJ -196.0 kJ +98.0 kJ +196.0 kJ more information needed

A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 189 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 °C. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures.

When a 3.25 g sample of solid sodium hydroxide was dissolved in a calorimeter in 100.0 g of water, the temperature rose from 23.9 C to 32.0 C. Calculate ΔH in kJ/mol NaOH) for the solution process: NaOH(s) --> Na+ (aq) + OH-(aq) Assume it's a perfect calorimeter and that the specific heat of the solution is the same as that of pure water.

The amount of space an object occupies may be found by h. mass f. length g. time i. volume Which of the following measurements is most precise? a. 5.432 C. 5.4 d. 5 b. 5.43

(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. Cr³+ (aq) + 3e- ---> Cr(s) Mn(s)→ Mn2+ (aq) + 2e- (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients.

Select all the statements that are true when magnesium reacts with chlorine: A. The compound that forms is MgCl B. Magnesium transfers electrons to chlorine C. Magnesium becomes a +2 cation D. Chlorine becomes a -2 anion DE. Chlorine transfers electrons to magnesium F. The formula for the compound formed is MgCl2 G. Chlorine becomes an anion

For the following electron-transfer reaction: Mn(s) + Cu²+ (aq) → Mn²+ (aq) + Cu(s) The oxidation half-reaction is: The reduction half-reaction is: Use the References to access important values if needed for this question. Enter electrons as e-. Use smallest possible integer coefficients. If a box is not needed, leave it blank.

When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown? F- + Br₂-> Br- + F2 Water appears in the balanced equation as a Which element is reduced? (reactant, product, neither) with a coefficient of (Enter 0 for neither.)

A raindrop has a mass of 50. mg and the Pacific Ocean has a mass of 7.08 × 10^20 kg. Use this information to answer the questions below. Be sure your answers have the correct number of significant digits. What is the mass of 1 mole of raindrops? Round your answer to 2 significant digits. How many moles of raindrops are in the Pacific Ocean? Round your answer to 2 significant digits.

A 14.0 g sample of an aqueous solution of hydrobromic acid contains an unknown amount of the acid. If 29.0 mL of 7.88×10-² M barium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass of hydrobromic acid in the mixture? % by mass

You have three known solutions: 1) Na₂CO3 2) BaCl2 3) KNO3 Even though you know that you have these three solutions, you do not know which one is which because they are not labeled. Which one of the following reagents should you add to each solution to be able to accurately identify and label them? Select one: A. We need more than one of these reagents to be able to identify all three solutions. B. CaCl2 C. H₂SO4 D. HCI E. NaOH

Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction. 3F2+2Al- →6F- +2A1³+ species oxidized oxidizing agent species reduced reducing agent As the reaction proceeds, electrons are transferred from _ to _

The gasoline in an automobile gas tank has a mass of 60.0 kg and a density of 0.752 g/mL A) What's the specific gravity B) Calculate the volume of gasoline in gallons (Show your calculations):

SnO₂²- + 2NH₂OH = SnO3²- + N₂H4+ H₂O In the above reaction, the oxidation state of tin changes from How many electrons are transferred in the reaction?

What volume of 2.5 M Nitric acid (HNO3) is required to prepare 500 mL of a 0.20 M HNO3 solution 40 mL 0.2 mL 500 mL 2.5 mL

Does a reaction occur when aqueous solutions of iron(II) iodide and lead(II) nitrate are combined? no yes If a reaction does occur, write the net ionic equation. Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank.

When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? I2 + Cl- ---> I- + Cl2 Water appears in the balanced equation as a (reactant, product, neither) with a coefficient of (Enter 0 for neither.) Which species is the oxidizing agent?

Iron(III) sulfide reacts with HCI (g) to produce iron(III) chloride and hydrogen sulfide. When 56.8 g of iron(III) sulfide reacts with 42.3 g of hydrochloric acid to produce 54.2 g of iron(III) chloride, what is the percent yield for the reaction? Molar masses: Fe (55.85 g/mol) S (32.07 g/mol) Cl (35.45 g/mol) H (1.008 g/mol) Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal place.

When the following half reaction is balanced under basic conditions, what are the coefficients of the species shown? NiO₂ + H₂O ---> Ni(OH)₂ + OH- In the above half reaction, the oxidation state of nickel changes from _ to _

When the following half reaction is balanced under acidic conditions, what are the coefficients of the species shown? Mn2+ H₂O ---> MnO₂ + H+ In the above half reaction, the oxidation state of manganese changes from _ to _

to access important values if needed for this question. When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? Br₂ NH₂OH = N2H4+ Br2 Water appears in the balanced equation as a0 for neither.) Which species is the reducing agent?

A solution contains 35 g of KBr dissolvedin 205 g of water. Express the concentration of the solution as % (m/m). 14.6 % (m/m) 12.3 % (m/m) 5.86 % (m/m) 17.1 % (m/m)

A 14.9 g sample of an aqueous solution of hydrochloric acid contains an unknown amount of the acid. If 16.0 mL of 1.03 M sodium hydroxide are required to neutralize the hydrochloric acid, what is the percent by mass of hydrochloric acid in the mixture? % by mass

You are exposed to a small amount of radiation daily. This small radiation exposure is the background radiation relative biological efficiency personal radiation inherent radiation

An unknown compound has the following chemical formula: P₂Ox where x stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 6.3 mol of oxygen and 2.50 mol of phosphorus. Write the complete chemical formula for the unknown compound.

How much energy in kilocalories is lost when a sample 225 mL water cools from 75.0°C to 22.0°C? (Specific Heat Capacity of water is 1.00 cal/g °C or 4.184 J/g°C) Density 1.00 g/mL (Show your calculations

What volume of a 0.170 M barium hydroxide solution is required to neutralize 27.3 mL of a 0.141 M perchloric acid solution? mL barium hydroxide

Calculate the mass percent of element A in a compound with molecular formula A2B3. The molar mass of element A is 35.5, and molar mass of element B is 48.5. When input answer, convert percentage to decimal. Use 3 decimal places. For example, if you answer is 56.7%, convert it to 0.567

The movie below shows some molecules in a tiny sample of a mixture of gases. Drag the slider to see how the molecules move. Does a chemical reaction happen during this movie? If a chemical reaction does happen, write a balanced chemical equation for it.

Magnesium metal, Mg (s), reacts with hydrochloric acid to form aqueous magnesium chloride and hydrogen gas. When 43.5 g of magnesium is added to 258 mL of 6.00 M hydrochloric acid, what mass (in grams) of hydrogen is produced, assuming the reaction goes to completion? Molar masses: Mg (24.31 g/mol) CI (35.45 g/mol) H (1.008 g/mol) Do NOT include units in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal places.

A 1.45-g sample of phosphorus burns in air and forms 2.57 g of a phosphorus oxide. Calculate the empirical for- mula of the oxide. (Hint: Determine the mass of oxygen in the 2.57 g of phosphorus oxide by determining the differ- ence in mass before and after the phosphorus burns in air.)

Solid iron and aqueous magnesium chloride are produced by the reaction of aqueous iron(III) chloride and solid magnesium. Write a balanced chemical equation for this reaction

A chemistry student weighs out 0.215 g of phosphoric acid (H₂PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits.

0.29 g sodium iodide reacts with chlorine, producing 0.075 g sodium chloride and some amount of iodine. Find the percent yield of NaCl. Write and balance the equation first. Don't forget diatomics and how to write formulas.

2.0 liters of ethanol (C₂H6O, density = 0.789 g/mL) combusts with 2.0 kilograms oxygen gas to produce carbon dioxide and water. What is the maximum mass of water than can form? Write the balance equation first.

Silver ion reacts with chloride ion to form the precipitate silver chloride: Ag+(aq)+C1-(aq) AgCl(s) After the reaction reached equilibrium, the chemist filtered 99% of the solid silver chloride fromthe solution, hoping to shift the equilibrium to the right, to form more product. Critique the chemist's experiment.