Inorganic Chemistry Questions

A chemist prepares a solution of potassium iodide (KI) by measuring out 6.1 × 10² μmol of potassium iodide into a 500. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's potassium iodide solution. Round your answer to 2 significant digits.

A chemist makes 430. mL of silver nitrate (AgNO3) working solution by adding distilled water to 170. mL of a 5.01 M stock solution of silver nitrate in water. Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits.

A chemist prepares a solution of aluminum sulfate (Al₂(SO4)3) by measuring out 43.8 g of aluminum sulfate into a 100. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's aluminum sulfate solution. Round your answer to 3 significant digits.

Identify the true statements about the magnetism of rocks on the sea floor. (Check all that apply.) Rocks contain tiny magnetic particles. Rocks that have cooled down change their orientation when the magnetic field changes. The rocks act like tiny compasses and always point north despite the direction of Earth's field. The orientation of Earth's magnetic field can be determined at the time the rocks cooled.

A chemist prepares a solution of calcium bromide (CaBr₂) by measuring out 57. μmol of calcium bromide into a 150. mL volumetric flask and filling the flask to the mark with water." Calculate the concentration in mol/L of the chemist's calcium bromide solution. Round your answer to 2 significant digits.

A mixture of CaCO3 and CaO weighing 0.693 g was heated to produce gaseous CO₂. After heating, the remaining solid weighed 0.508 g. Assuming all the CaCO3 broke down to CaO and CO2, calculate the mass percent of CaCO3 in the original mixture.

In a car engine, gasoline (represented by C8H18) does not burn completely, and some CO, a toxic pollutant, forms along with CO₂ and H2₂O. If 5.0% of the gasoline forms CO: (a) What is the ratio of CO₂ to CO molecules in the exhaust? (b) What is the mass ratio of CO₂ to CO? (c) What percentage of the gasoline must form CO for the mass ratio of CO₂ to CO to be exactly 1/1?

Give the spectroscopic notation (also called spdf notation) electron configuration of F Enter the subshells in the order in which they are filled. For example, for oxygen, the answer would be: 1s22s22p4.

In a beaker, 0.86 mol of potassium iodide and 0.52 mol of lead (II) nitrate are dissolved in water. A reaction occurs, and a white precipitate is observed. Calculate the mass (in grams) of the precipitate formed. Assume the reaction goes to completion. 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.

What is the mass of boron (in g) in a 27.5g sample of boric acid, B(OH)3? Note: For the formula weight, use the values from our periodic table. Round your answer to 4 significant figures, do not include units.

Aluminum sulfate, known as cake alum, has a wide range of uses, from dyeing leather and cloth to purifying sewage. In aqueous solution, it reacts with base to form a white precipitate. (a) Write balanced total and net ionic equations for its reaction with aqueous NaOH. (b) What mass of precipitate forms when 185.5 mL of 0.533 M NaOH is added to 627 mL of a solution that contains 15.8 g of aluminum sulfate per liter?

In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 20.00 mL of 0.0502 M NaOH but overshoot the end point, and the solution turns deep pink. Instead of starting over, you add 30.00 mL of the acid, and the solution turns colorless. Then, it takes 3.22 mL of the NaOH to reach the end point. (a) What is the concentration of the HNO3 solution? (b) How many moles of NaOH were in excess after the first addition?

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. Answer:

Give the "box notation" (also called the "dash notation") electron configuration of Ca by filling electrons into the orbital spaces provided. Press Check when complete.

Magnesium metal, Mg (s), reacts with water, H₂O (l), to form magnesium hydroxide and hydrogen gas, H₂ (g). What mass of hydrogen gas can be produced in the reaction of 146.0 g of magnesium with 193.3 g of water? Assume the reaction goes to completion and that it occurs at room temperature and pressure. Molar mass: for the hydrogen atom, H, must use 1.008 g/mol. Thus, for H₂ (g) use 2.016 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.

How many electrons are transferred in the following oxidation-reduction reaction? Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) a. 1 b. 3 C. 4 d. 2 e. 5

Ammonia is produced by the millions of tons annually for use as a fertilizer. It is commonly made from N₂ and H₂ by the Haber process. Because the reaction reaches equilibrium before going completely to product, the stoichiometric amount of ammonia is not obtained. At a particular temperature and pressure, 10.0 g of H₂ reacts with 20.0 g of N₂ to form ammonia. When equilibrium is reached, 15.0 g of NH3 has formed. (a) Calculate the percent yield. (b) How many moles of N₂ and H₂ are present at equilibrium?

Ammonia gas reacts with oxygen gas, O₂(g), to produce nitrogen dioxide and water. When 28.5 g of ammonia gas reacts with 83.4 g of oxygen gas to produce 62.6 g of nitrogen dioxide, what is the percent yield of the reaction? Molar mass: for the hydrogen atom, H, must use 1.008 g/mol and for the nitrogen atom, N, use 14.01 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.

Consider the following chemical reaction: 3 H₂ + N₂ --> 2 NH3 If 3.50 g of H₂ reacts with 21.0 g of N₂ to produce 18.8 g of NH3, what is the percent yield of NH3? Molar mass: for the hydrogen atom, H, must use 1.008 g/mol and for the nitrogen atom, N, use 14.01 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.

How many moles of solute are present in 300.0 mL of a 7.6 M solution of NaOH (aq)? 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. Answer:

Using NOBLE GAS notation write the electron configuration for the scandium atom.

Give the electron configurations for P and Pb using the short-hand, noble gas method. For example, the electron configuration 1s22s22p63s23p2 (for silicon) is [Ne]3s²3p²

Write the complete electron configuration for the helium atom. Using NOBLE GAS notation write the electron configuration for the beryllium atom.

Complete and balance the molecular equation for the reaction of aqueous chromium(II) bromide, CrBr₂, and aqueous sodium carbonate, Na₂CO3. Include physical states. molecular equation: Enter the balanced net ionic equation for the reaction. Include physical states. net ionic equation:

What factors are required for a molecule to be polar? (Choose all that apply) The presence of polar covalent bonds are required. Polar bonds must be symetrically arranged around the central atom. Polar bonds must be assymetrically arranged around the central atom. There must be two or more polar bonds on the central atom. The central atom must have a non-bonding pair of electrons. The dipoles must add up to result in a net dipole.

Liquid hexane (CH₂(CH₂)4CH3) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 6.9 g of hexane is mixed with 39.2 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.

A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of product. Calculate the empirical formula of the iron sulfide.

Write the complete electron configuration for the neon atom. Using NOBLE GAS notation write the electron configuration for the carbon atom.

Write the complete electron configuration for the sodium atom. Using NOBLE GAS notation write the electron configuration for the lithium atom.

The heat of combustion of fructose, C6H12O6, is -2812 kJ/mol. If a fresh golden delicious apple weighing 4.21 oz (119 g) contains 16.0 g of fructose, what caloric content does the fructose contribute to the apple? Express your answer in Calories to three significant figures.

Even though thermodynamically favourable, the conversion of diamond into graphite does not occur normally since. the activation energy of the process is high. the activation energy of the process is low. the change of entropy is zero. the change of enthalpy is zero.

Gaseous butane (CH₂(CH₂)2CH₂) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 0.58 g of butane is mixed with 3.91 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: BrO3-, CH3CO₂-, Fe3+, NH4+

81. (77 in the 3rd edition) Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4(g) + H₂O(g) -> CO(g) + 3 H₂(g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

The solubility rules are listed in table below. General Rules for Solubility of lonic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3) salts are soluble. 2. Most salts of Na+, K+, and NH4+ are [soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl2. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble. The important exceptions are NaOH and KOH: Ba(OH)2 and Ca(OH)2 are only moderately soluble, 6. Most sulfide (S2), carbonate (CO32), and phosphate (PO4) salts are only slightly soluble." "The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. On the basis of the general solubility rules, choose the substance that is not likely to be soluble in water. a. K₂SO3 PbSO3 Na₂SO3 C8₂SO3 b. BaF₂ CsF KF NaF C.KF CaF₂ NaF CsF

From the list below, choose which groups are part of the periodic table. metals acids flammable gases nonmetals semimetals ores conductors

A 25.00 mL sample of 6.00 M HCl solution is diluted to a new volume of 85.00 mL. What is the concentration of the dilute solution? 0.568 M 2.82 M 2.04 M 1.76 M I DON'T KNOW YET

A solution involves an attraction between the solute, the substance being dissolved, and the solvent, the substance that does the dissolving. This attraction is based on the polarity of the solute and the solvent. a. If both the solute and the solvent are polar, the solute will dissolve in the solvent. The same can also be said the solute and the solvent are nonpolar. This results in the formation of a solution. b. However, if the solute and the solvent have differing polarities (i.c., one is polar and the other is nonpolar), they will not dissolve in one another, and a solution will not form. Which substance will dissolve in water? CCI4 C4H10 CH3OH BF3 I DON'T KNOW YET

Aluminium chloride exists as a dimer, Al2Cl6 in solid state as well as in solution of non-polar solvents such as benzene. When dissolved in water it gives:

1. Using chemical formulas, write out the equations of the three reactions you will do, then balance. 2. Classify the reactions as synthesis, decomposition, single displacement or double displacement. Note: the first reaction is a redox reaction and does not fall into any one of the other four categories. (1) Redox. (2) (3) 3. During reaction 1, a brown gas is produced. What is its formula? 7. Reaction 2 involves combining a solution of sodium hydroxide with a solution of copper (II) nitrate. The sodium hydroxide solution is colorless. a. What color is the copper (II) nitrate solution? b. What species is responsible for this color? How do you know when reaction 3 is complete? A student started with 0.3295 g of copper. The mass of filter paper and copper (II) oxide product was found to be 0.5723 g, and that of the filter paper alone was 0.2568 g. Calculate the percent yield of copper (II) oxide.

An inorganic compound (A) is white and exist as dimer. (A)Get sublimes on Heating (A)Gives fumes (B) with wet air (A) Gives white ppt with NH₂OH. However (A) Is soluble in excess of NaOH to give soluble compound (C) The inorganic compound 'A's Al₂O3 AlBr3 AICI 3 BeCl₂ An inorganic compound (A) is white and exist as dimer. (A)Get sublimes on Heating (A)Gives fumes (B) with wet air (A) Gives white ppt with NH₂OH. However (A) Is soluble in excess of NaOH to give soluble compound (C) The soluble compound (C) NaBO₂ NaAlO₂ Al₂O3 Al(OH)3

(CH₂(CH₂)4CH3) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 37.9 g of hexane is mixed with 99. g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.

53.1 g of calcium sulfate dihydrate, gypsum, is heated in an oven until all the water is driven off. What is the mass of the anhydrous compound? Provide your answer in decimal notation rounded to the appropriate number of significant figures.

1.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 138. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: Use this information to find the molecular formula of X.

A 32.9 mL sample of Ba(OH), is titrated with HCl. If 37.2 mL of 0.863 M HCl is needed to reach the endpoint, what is the concentration (M) of the Ba(OH), solution? Ba(OH)₂ (aq) + 2 HCl(aq) → BaCl(aq) + 2 H₂O(l) 0.382 M 0.488 M 0.976 M 1.95 M I DON'T KNOW YET

Ammonium perchlorate (NH4CIO4) is a powerful solid rocket fuel, used in the Space Shuttle boosters. It decomposes into nitrogen (N₂) gas, chlorine (Cl₂) gas, oxygen (0₂) gas and water vapor, releasing a great deal of energy. Calculate the moles of oxygen produced by the reaction of 1.3 mol of ammonium perchlorate. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Adding base to pure water causes the [OH-] to equilibrium for water to shift in the direction toward the The shift causes the [H3O+] to [H3O+] x [OH-], which equals This added stress causes the and away from the in order to maintain the product

In a solution of pure water, the dissociation of water can be expressed by the following: H₂O(l) + H₂O(l) H₂O'(aq) + OH(aq) The equilibrium constant for the ionization of water, K, is called the ion-product of water. In pure water at 25 °C, K has a value of 1.0 10¹. The dissociation of water gives one H₂O' ion and one OH ion and thus their concentrations are equal. The concentration of each is 1.0 x 10 M. K - [HO][OH^] K(1.0 10 )(1.0 × 10) - 1.0 × 10 ¹¹ X X [H₂O'][OH]- 1.0 × 10 ¹ X A solution has a [OH ]-3.4 10 M at 25 °C. What is the [HO] of the solution? O O 2.9 × 109 M X 3.4 × 10⁹ M 2.9 × 10-¹5 M 2.9 × 10 10 M I DON'T KNOW YET

Compound X has a molar mass of 180.15 g mol and the following composition: element mass % carbon hydrogen 6.71% oxygen 40.00% 53.29% Write the molecular formula of X.

Hydrogen sulfide gas (H₂S) and aqueous iron(II) chloride are formed by the reaction of aqueous hydrochloric acid (HCI) and solid iron(II) sulfide