Inorganic Chemistry Questions

The name of the 7th most abundant gas in dry air at sea level is

The energy content of food is typically determined using a bomb calorimeter. Consider the combustion of a 0.24-g sample of butter in a bomb calorimeter having a heat capacity of 2.67 kJ/°C. If the temperature of the calorimeter increases from 23.5°C to 26.0°C, calculate the energy of combustion per gram of butter.

A gaseous mixture containing 1.5 mol Ar and 3.5 mol CO₂ has a total pressure of 9.5 atm. What is the partial pressure of CO₂? 22 atm 1.8 atm 9.5 atm 6.7 atm 2.9 atm

Which of the following properties of a real gas is related to the b coefficient in the van der Waals equation? The average speed of the molecules of a real gas increases with temperature. Real gases consist of molecules or atoms that have volume. There are attractive forces between atoms or molecules of a real gas. The rate of effusion of a gas is inversely proportional to the square root of the molecular weight of the gas. None of these choices are correct.

A newly discovered gas has a density of 2.33 g/L at 25.0 °C and 709 mm Hg. What is the molar mass of the gas? 61.1 g/mol 5.13 g/mol 805 g/mol 11.3 g/mol

A compound is found to contain 30.45 % nitrogen and 69.55 % oxygen by mass. The empirical formula for this compound is The molar mass for this compound is 46.01 g/mol. The molecular formula for this compound is

Methanol (CH3OH) has been proposed as an alternative fuel. Calculate the standard enthalpy of combustion per gram of liquid methanol. Standard Heats of Formation: CH3OH(l) = -239 kJ/mol O2(g) = 0 kJ/mol CO2(g)=–393.5 kJ/mol H₂O(l) = -286 kJ/mol

1. How many MOLECULES of boron tribromide are present in 3.50 moles of this compound? 2. How many MOLES of boron tribromide are present in 1.04×10^23 molecules of this compound?

A mixture of nitrogen and krypton gases, in a 8.91 L flask at 52 °C, contains 5.43 grams of nitrogen and 20.4 grams of krypton. The partial pressure of krypton in the flask is ___ atm and the total pressure in the flask is ___atm.

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

It is desired to inflate a baggie with a volume of 912 milliliters by filling it with neon gas at a pressure of 0.965 atm and a temperature of 309 K. How many grams of Ne gas are needed?

Calculate the percentage composition for XeO3. Mass percentage of xenon Mass percentage of oxygen

You have a certain mass of helium gas (He) in a rigid steel container. You add the same mass of neon gas (Ne) to this container. Which of the following best describes what happens? Assume the temperature is constant. The pressure in the container more than doubles. The pressure in the container doubles. The volume of the container more than doubles. The volume of the container doubles. The pressure in the container increases but does not double.

Oxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KC1O3(s)- +2KCI(s) + 3O2(g) The product gas, O₂, is collected over water at a temperature of 20 °C and a pressure of 745 mm Hg. If the wet O₂ gas formed occupies a volume of 8.57 L, the number of grams of O₂ formed is g. The vapor pressure of water is 17.5 mm Hg at 20 °C.

A sample of hydrogen gas has a density of _____ g/L at a pressure of 1.08 atm and a temperature of 33 °C.

A 9.200 mol sample of methane gas is maintained in a 0.8079 L container at 304.2 K. What is the pressure in atm calculated using the van der Waals' equation for CH4 gas under these conditions? For CH4, a= 2.253 L²atm/mol² and b= 4.278x10-² L/mol.

A sample of neon gas occupies a volume of 7.86 L at 59.0°C and 0.900 atm. If it is desired to increase the volume of the gas sample to 9.04 L, while increasing its pressure to 1.08 atm, the temperature of the gas sample at the new volume and pressure must be ___

Calculate the internal energy change for each of the following. a. One hundred (100.) joules of work is required to compress a gas. At the same time, the gas releases 46 J of heat. Internal energy change = Piston is compressed from a volume of 5.05 L to 1.15 L against a constant pressure of 3.70 atm. In the process, there is a heat gain by the system of 671 J. Internal energy change = c. A piston expands against 2.05 atm of pressure from 19.0 L to 31.4 L. In the process, 1687 J of heat is absorbed. Internal energy change =

In a chemical analysis of a chromium alloy, all of the chromium is first converted to chromate ions. A 50.0 mL sample of the chromate ion solution is then reduced in a basic solution to chromium(III) hydroxide by reaction with 22.6 mL of 1.08 mol/L sodium sulfite. In this reaction, the sulfite ions are oxidized to sulfate ions. What is the amount concentration of the chromate ion solution?

What volume of hydrogen gas is produced when 58.4 g of iron reacts completely according to the following reaction at 25 °C and 1 atm? iron (s) + hydrochloric acid(aq)-iron(II) chloride (aq) + hydrogen(g)

Real gases are those that: Oare only available naturally in the earth's atmosphere. Oonly behave ideally at high pressures or low temperatures. have an even number of protons. are called real gases because their behavior can easily be modeled. deviate from ideal behavior.

You carry out the synthesis of Ca(OH)2 using the 2.04 g of KOH and 3.02 g of CaCl2-2H₂O as in #1, and your yield of dry Ca(OH)2 is 1.22 g. What is the percent yield for the reaction?

A sealed balloon is filled with 1.00 L helium at 22°C and 1.00 atm. The balloon rises to a point in the atmosphere where the pressure is 30.7 torr and the temperature is -55°C. What is the change in volume of the balloon as it ascends from 1.00 atm to a pressure of 30.7 torr?

A mixture of carbon dioxide and neon gases is maintained in a 6.37 L flask at a pressure of 3.14 atm and a temperature of 25 °C. If the gas mixture contains 13.6 grams of carbon dioxide, the number of grams of neon in the mixture is __g.

A 149.3-g sample of a metal at 75.1°C is added to 149.3 g H₂0 at 14.6°C. The temperature of the water rises to 18.8°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C-g-

The van der Waals equation, nRT = [P+ a(n/V)2] (V-nb), incorporates corrections to the ideal gas law in order to account for the properties of real gases. One of the corrections accounts for the quantum behavior of molecules. the possibility of chemical reaction between molecules. the possibility of phase changes when the temperature is decreased or the pressure is increased. the fact that average kinetic energy is inversely proportional to temperature. Othe finite volume of molecules.

A 5.78 gram sample of neon gas has a volume of 912 milliliters at a pressure of 3.95 atm. The temperature of the Ne gas sample is

Oxygen gas, generated by the reaction 2KCIO3(s) → 2KCl(s) + 30₂(g) is collected over water at 27°C in a 3.27-L vessel at a total pressure of 1.00 atm. (The vapor pressure of H₂at 27°C is 26.0 torr.) How many moles of KCIO3 were consumed in the reaction? 0.0855 moles 0.192 moles O3.16 moles 0.0916 moles 0.128 moles

Boyle's law states that: The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure. Equal amounts of gases occupy the same volume at constant temperature and pressure. The rates of effusion of gases are inversely proportional to the square roots of their molar masses. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds. The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

You fill a balloon with 2.50 moles of gas at 27°C at a pressure of 1.92 atm. What is the volume of the balloon? 18.9 L 2.84 L 32.0 L 22.4 L 118 L

Compute the root-mean-square speed of He molecules in a sample of helium gas at a temperature of 183°C.

The pressure of the atmosphere decreases with increasing altitude in the Choose all that apply. stratosphere thermosphere troposphere mesosphere The pressure never decreases with increasing altitude.

Which of the following is true about the kinetic molecular theory? Pressure is due to the collisions of the gas particles with the walls of the container. The volume of a gas particle is considered to be small about 0.10 mL. Gas particles repel each other, but do not attract one another. Adding an ideal gas to a closed container will cause an increase in temperature. At least two of these statements are correct.

The name of the 11th most abundant gas in dry air at sea level is

In which of these layers of the atmosphere does the temperature increase with increasing altitude? Choose all that apply. Stratosphere Thermosphere Troposphere Mesosphere

Which of the following statements is true for real gases? As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas. As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas.

Which of the following would represent the greatest pressure? 15.5 in Hg 0.660 atm 0379 mmHg 067055 Pa 12.9 psi

When elemental copper is strongly heated with sulfur, a mixture of CuS and Cu₂S is produced, with CuS predominating. Cu(s) + S(s) → CuS(s) 2Cu(s) + S(s) → Cu₂S(s) What is the theoretical yield of CuS when 33.70 g of Cu(s) is heated with 45.80 g of S? (Assume only CuS is produced in the reaction.) Theoretical yield = What is the percent yield of CuS if only 36.2 g of CuS can be isolated from the mixture? Percent yield =

A mixture of neon and xenon gases at a total pressure of 716 mm Hg contains neon at a partial pressure of 429 mm Hg. If the gas mixture contains 2.78 grams of neon, how many grams of xenon are present?

A sample of neon gas at a pressure of 987 mm Hg and a temperature of 59 °C, occupies a volume of 11.6 liters. If the gas is cooled at constant pressure to a temperature of 30 °C, the volume of the gas sample will be ___ L.

A mixture of nitrogen and krypton gases, at a total pressure of 768 mm Hg, contains 4.19 grams of nitrogen and 15.8 grams of krypton. What is the partial pressure of each gas in the mixture?

A sample of nitrogen gas at a pressure of 0.615 atm and a temperature of 210 °C, occupies a volume of 574 mL. If the gas is cooled at constant pressure until its volume is 485 mL, the temperature of the gas sample will be ___ °C.

A sample of carbon dioxide gas collected at a pressure of 324 mm Hg and a temperature of 284 K has a mass of 54.6 grams. The volume of the sample is ___ L.

Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the reaction of an acid on an alkaline earth metal peroxide, such as barium peroxide. BaO2 (s) + HCl(aq) → H₂O₂ (aq) + BaCl₂ (aq) What amount of hydrogen peroxide should result when 1.18 g of barium peroxide is treated with 26.7 ml of hydrochloric acid solution containing 0.0283 g of HCI per mL?

The rate of effusion of O₂ gas through a porous barrier is observed to be 3.45 x 10^-4 mol/h. Under the same conditions, the rate of effusion of O3 gas would be ___ mol/h.

A sample of O₂ gas is observed to effuse through a pourous barrier in 3.56 minutes. Under the same conditions, the same number of moles of an unknown gas requires 2.48 minutes to effuse through the same barrier. The molar mass of the unknown gas is ___ g/mol.

For each of the following problems, show your calculation setup. In both your setup and answer, show units and follow the rules of significant figures. 1. Convert 78°F to degrees Celsius

When aqueous solutions of chromium(II) nitrate and ammonium carbonate are combined, solid chromium(II) carbonate and a solution of ammonium nitrate are formed. The net ionic equation for this reaction is:

Write the balanced net ionic equation for the precipitation of zinc sulfide from aqueous solution:

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