Inorganic Chemistry Questions

A. What is the hybridization of the central atom in ICl5? Hybridization = What are the approximate bond angles in this substance ? Bond angles = B. What is the hybridization of the central atom in XeF₂? Hybridization = What are the approximate bond angles in this substance? Bond angles =

3. Find the molar mass of (a) nitric acid, HNO3; (b) nickel (II) nitrate, Ni(NO3)2; and (c) potassium hydrogen carbonate, KHCO3 (a) (b) (c)

Absent any form of central authority after the fall of Rome, people in Western Europe were paying up to three quarters of their income for ______. A. food B. taxes C. medical attention D. protection

A. What is the hybridization of the central atom in SF4? Hybridization = What are the approximate bond angles in this substance ? Bond angles = B. What is the hybridization of the central atom in BrF5? Hybridization = What are the approximate bond angles in this substance ? Bond angles =

9. A water solution of sulfuric acid has a density of 1.67 grams/mL and is 75 percent H₂SO4 by mass. How many moles of H₂SO4 are contained in 400 mL of this solution?

A coffee cup calorimeter is filled with 200.0 mL of water at 22.1°C. A piece of metal at 48.6° C with a mass of 5.1 g is added. The final temperature of the water in the calorimeter is 26.8°C. The density of liquid water is 1.00 g/mL, and its specific heat capacity is 4.18 J/(g°C). Determine the specific heat capacity of the metal. Place your final answer in blank #1.

The chemical reaction system that can be used to produce the biofuel methanol, CH3OH (g),is represented by the following equation: 2 H2(g) + CO (g) = CH3OH (g) K = 10.5 at 500 K Question #1) When the concentrations of hydrogen, H2 (g); carbon monoxide, CO (g); and methanol are 0.25 mol/L, 0.25 mol/L, and 0.040 mol/L, respectively, is the system at equilibrium? Place your answer in blank #1. Question #2) If not, predict the direction in which the equilibrium will shift and explain why. Place your answer in blank #2.

To which of the following types of reactions do we apply Le Chatelier's principle? all reactions at equilibrium reversible reactions all chemical reactions precipitation reactions none of the above

Fe³+ (aq) + SCN¹-(aq) <======> FeSCN¹-(aq) (colourless) (brown) (deep red) What is observed if a few drops of iron (III) chloride is added to this equilibrium? nothing happens it becomes darker red none of the above it becomes lighter red becomes colourless

In the reaction represented by the general equation: A + 2B 3C + 4D the initial concentration of B was 0.0431 mol/L. After 11.3 minutes, the concentration of B was 0.0307 mol/L. a) Calculate the average rate of consumption of B for the first 11.3 minutes in mol/(Ls). Put your answer in the first blank. b) Calculate the average rate of formation of C. Put your answer in the second blank.

Chemical kinetics is the study of factors that affect the rate of a chemical reaction the chemical properties of substances the rate of a change in concentration the physical properties of substances none of the above

A chemist must dilute 45.7 mL of 909. mM aqueous iron(II) bromide (FeBr₂) solution until the concentration falls to 203. mM. She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Be sure your answer has the correct number of significant digits.

A sample of an unknown sulfate compound has a mass of 0.100 g. Addition of excess barium chloride solution to the sample forms a barium sulfate precipitate of mass 0.0676 g. What is the mass % of sulfate ion in the unknown sample?

A sample of mercury (II) bromide, HgBr2, weighs 8.65 grams. How many moles are in this sample?

A sample of oxygen gas, O2 weighs 28.4 grams. How many molecules of O2 and how many atoms of O are present in this sample?

Indicate whether each of the following describes a gas, a liquid, or a solid. The substance has no definite volume or shape The particles in a substance do not interact with each other The particles in a substance are held in a rigid structure

a. Identify the element that has atomic nuclei represented by nucleus 1. b. Explain why nucleus 2 and nucleus 4 represent the nuclei of two different isotopes of the same element. c. Identify the nucleus above that is found in an atom that has a stable valence electron configuration.

Which of the following pairs of gas samples would have closest to the same number of particles? A. 73.1 g of SF6 and 1.0 g of H₂ B. 8.8 g of CO₂ and 10.4 g of C3H8 C. 10.8 g of Ne and 36.0 g of Kr D. 4.0 g of O₂ and 4.0 g of N₂

In a coffee-cup calorimeter, 1.56 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.22°C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.36°C. Assuming the solution has a heat capacity of 4.18 J/°C-g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.

A chemist adds 415.0 mL of a 8.15 x 10-5 mol/L zinc oxalate (ZnC₂O4) solution to a reaction flask. Calculate the micromoles of zinc oxalate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Describe each of the following as a physical (P) or chemical property (C). Chromium is a steel-gray solid. Hydrogen reacts readily with oxygen. Nitrogen freezes at -210 degrees Celsius. Milk will sour when left in a warm room.

A 29.3-g sample of water at 300. K is mixed with 50.7 g water at 350. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.

Calculate ΔH for the reaction: 2NH3 (g) + O2(g) → N₂H₁ (l) + H₂O(l) given the following data: 2NH3(g) + 3N₂O(g) → 4N2 (g) + 3H₂O(l) ΔH-1010kJ N₂O(g) + 3H₂(g) → N₂H4 (1) + H₂O(l) ΔH = -317 kJ N₂H4 (l) + O2(g) → N₂(g) + 2H₂O(l) ΔH=-623 kJ H2(g) + 1/2 O2(g) → H₂O(l) ΔH-286 kJ

For the following reaction, 55.4 grams of potassium hydrogen sulfate are allowed to react with 21.5 grams of potassium hydroxide. potassium hydrogen sulfate(aq) + potassium hydroxide(aq) → potassium sulfate(aq) + water(l) What is the maximum amount of potassium 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?

When 170. J of heat are absorbed by 150. g of copper at 23.61 °C, the temperature increases to 26.51 °C. What is the specific heat of copper?

Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction: 2NaN3 (s) → 2 Na(s) + 3N₂(g) What mass of NaN3 (s) must be reacted to inflate an air bag to 68.0 L at STP?

Helium is collected over water at 25°C and 1.00 atm total pressure. What total volume of gas must be collected to obtain 0.487 g helium? (At 25°C the vapor pressure of water is 23.8 torr.)

Calculate the mass (in amu) of a sample of iron (Fe) that contains 15 atoms Calculate the number of copper (Cu) atoms present in a sample that has a mass of 1779.4 amu Calculate the number of moles of atoms and the number of atoms in a 25.0g sample of calcium Calculate the molar mass of ammonia (NH3) and sodium carbonate (Na2CO3) How many moles of tetraphosphorus decoxide (P4010) does a 250.0g sample represent?

Which of the following statements about chemical formulas is FALSE? The subscripts represent the relative mass of each type of atom in the compound. The subscripts do not change for a given compound. The subscripts represent the relative number of each type of atom in the compound. Different compounds made of the same elements have different subscripts.

Consider separate 1.0-L samples of Kr(g) and UFG (g), both at 1.00 atm and containing the same number of moles. What ratio of temperatures for the two samples would produce the same root mean square velocity?

Identify each of the following as a physical (P) or chemical properties (C) of a candle: A candle is 10 in. high and 2 in. in diameter The wax of a candle softens on a hot day A candle burns The candle is blue

An aerosol can contains 380. mL of compressed gas at 4.80 atm. When all of the gas is sprayed into a large plastic bag, the bag inflates to a volume of 1.90 L. What is the pressure of gas in the plastic bag? Assume a constant temperature.

Consider the following chemical equation: 2NO2(g) → N₂O4(g) If 50.0 mL NO2 gas is completely converted into N₂O4 gas under the same conditions, what volume will the N₂O4 occupy?

Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C4H4 (-2341 kJ/mol), C4H8 (-2755 kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction. C4H4 (g) + 2 H₂(g) → C4H4 (g)

Does a reaction occur when aqueous solutions of iron(III) sulfate and calcium chloride are combined? yes/no If a reaction does occur, write the net ionic equation.

When elements combine to form compounds: their properties are an average of all elements in the compound. their properties do not change. their properties are completely random. their properties change completely.

Methanol (wood alcohol) is a fuel that can be made from biomass (such as cellulose obtained from aspen trees). Methanol can also be made from natural gas. The overall synthesis reaction for the latter case is CH4(g) + H₂O() → CH₂OH(1) + H₂(g), ΔHo = ? Use the reactions below and Hess' law to predict the standard molar enthalpy of synthesis of methanol by this process. CO(g) + 3 H₂(g) -> CH4(g) + H₂O (l) ΔH = -249.9 kJ CO(g) + 2 H₂(g) → CH₂OH (l) ΔH"=-128.7 kJ

The element sodium forms a ____ with the charge ___ The symbol for this ion is ___ and the name is ___ ion. The number of electrons in this ion is ____

A sample of an ideal gas at 22.2 atm and 11.4 L is allowed to expand against a constant external pressure of 1.17 atm at a constant temperature. Calculate the work in units of kJ for the gas expansion. (Hint. Boyle's law applies.)

A 12.69 gram sample of iron is heated in the presence of excess chlorine. A metal chloride is formed with a mass of 36.85 g. Determine the empirical formula of the metal chloride.

Which of the following statements about the mole is FALSE? One mole of water contains 1/2 mole of oxygen atoms. One mole of a monatomic element has a mass equal to its atomic mass expressed in grams. A mole of a monatomic element corresponds to one Avogadro's number of atoms. One mole of atoms makes up an amount of atoms that can be seen with the naked eye.

Calculate the root mean square velocity for the O₂ molecules in a sample of O₂ gas at 11.8°C. (R = 8.3145 J/K mol) 471 m/s 95.9 m/s 9.88x10^26 m/s O272 m/s 14.9 m/s

An unknown diatomic gas has a density of 3.164 g/L at STP. What is the identity of the gas?

Uranium hexafluoride is a solid at room temperature, but it boils at 56°C. Determine the density of uranium hexafluoride at 70.°C and 735 torr.

Consider three 1-L flasks at STP. Flask A contains NH3 gas, flask B contains NO₂ gas, and flask C contains N₂ gas. Which contains the largest number of molecules? Flask C Flask A Flask B All are the same. More information is need to answer this.

N₂O is a gas commonly used to help sedate patients in medicine and dentistry due to its mild anesthetic and analgesic properties; it is also nonflammable. If a cylinder of N₂O is at 10.1 atm and has a volume of 6.50 L at 298 K, how many moles of N₂O gas are present? The gas from the cylinder is emptied into a large balloon at 755 torr. What is the volume of the balloon at 298 K?

A mixture of 1.40 g H₂ and 1.30 g He is placed in a 1.00-L container at 23°C. Calculate the partial pressure of each gas and the total pressure. PH₂ PHe PTOTAL

The name of the 8th most abundant gas in dry air at sea level is

When aqueous solutions of chromium(III) sulfate and sodium phosphate are combined, solid chromium(III) phosphate and a solution of sodium sulfate are formed. The net ionic equation for this reaction is:

Calculate the number of liters of oxygen that are needed to react with 310. mL of CH4 at 80.0 °C and 790 mm Hg in a complete combustion reaction. 0.155 L 0.620 L 6.20×10^5 L 620 L