Inorganic Chemistry Questions

If a gas at 0.832 atm pressure in a volume of 0.565 L is compressed to 0.195 L, what is the new pressure according to the ideal gas law? 0.287 atm 2.41 atm 3.48 atm 0.415 atm

a. Do the proton and the neutron have exactly the same mass? b. How do the masses of the proton and the neutron compare to the mass of the electron? c. Which particles make the greatest contribution to the mass of an atom? (Select all that apply.) protons neutrons electrons

Calculate the percent by mass of each element in the following compounds. HClO2

What volume of bromine monochloride is produced when 24.5 liters of bromine react according to the following reaction? (All gases are at the same temperature and pressure.) bromine(g) + chlorine(g) → bromine monochloride(g)

A scientist measures the standard enthalpy change for the following reaction to be -222.0 kJ: 2H₂O₂(I)→ 2H₂O(l) + O₂(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(I) is ___ kJ/mol.

Suppose you have a sample of sodium weighing 14.00 g. How many atoms of sodium are present in the sample? What mass of potassium would you need to have the same number of potassium atoms as there are sodium atoms in the sample of sodium?

A 162-mL sample of gas is collected over water at 22°C and 753 torr. What is the volume of the dry gas at STP? (The vapor pressure of water at 22°C = 20. torr) 142 mL 182 mL 149 mL 129 mL none of these

For a particular process q = -17 kJ and w = 21 kJ. Which of the following statements is false? The system does work on the surroundings. Heat flows from the system to the surroundings. ΔE = +4 KJ The process is exothermic. None of these choices is false.

A sample of gas contains 0.1500 mol of CH4(g) and 0.3000 mol of O₂(g) and occupies a volume of 14.7 L. The following reaction takes place: CH4(g) +20₂(g) → CO₂(g) + 2H₂O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

In a gas thermometer (constant pressure conditions) the gas has a volume of 1.00 L at 85.0 °C. The thermometer is placed in a freezer. The final volume measured is 0.29 L. What is the temperature of the freezer? 100 K 25 K 1.2×10³ K 3.4×10-³ K

A graduated cylinder was filled to 25.0 mL with liquid. A solid object weighing 73.5 grams was immersed in the liquid, raising the liquid level to 43.9 mL. Calculate the density of the solid object.

A binary compound of carbon and hydrogen has the following percentage composition: 79.89% carbon, 20.11% hydrogen by mass. If the molar mass of the compound is determined by experiment to be between 30 and 31 g/mol, what are the empirical and molecular formulas of the compound? Empirical formula: Molecular formula:

If you were travelling outward from the earth in a space shuttle at an altitude of 38.3 km you would be in the ____________

Write the formula and calculate the molar mass for each of the following compounds. a. iron(II) chloride Formula: Molar mass= b. calcium sulfate Formula: Molar mass= c. copper(II) chloride Formula: Molar mass=

A sample of an unknown gas is found to have a density of 1.99 g/L at a pressure of 0.732 atm and a temperature of 43 °C. The molar mass of the unknown gas is ___ g/mol.

Use the thermochemical data that follow to calculate the value of AH° for the reaction: 4B -> 2A+ C +2F ΔH° = 60 kJ A + 2B → E ΔH° = -40 kJ C+2D -> 2E ΔH° = 45 kJ F + 2A -> D 55 kJ 170 kJ 70 kJ -170 KJ -65 KJ

How many grams of iron are needed to completely consume 3.17 L of oxygen gas according to the following reaction at 25 °C and 1 atm? iron (s) + oxygen (g) iron(II) oxide (s)

A 1.29 mol sample of O₂ gas is confined in a 32.4 liter container at 33.5 °C. If 1.29 mol of H₂ gas is added holding the volume and temperature constant, the average molecular speed of the total system will remain the same increase decrease not enough information to answer the question

A 0.771 mol sample of He gas is confined in a 18.4 liter container at 18.2 °C. If 0.771 mol of CO₂ is substituted for the 0.771 mol of He, holding the volume and temperature constant, the average kinetic energy will increase decrease not enough information to answer the question remain the same

In the following 2-D illustrations, assume that the gas molecules are in motion and that if there is a larger box it indicates a larger volume for the container holding the molecules. A 30 molecules B 10 molecules If both gas samples are at the same pressure, the sample in box A has the highest temperature. both samples are at the same temperature. it is not possible to say anything about the relative temperatures. the sample in box B has the highest temperature.

A sample of gas contains 0.1900 mol of C₂H4(g) and 0.1900 mol of H₂O2(g) and occupies a volume of 15.2 L. The following reaction takes place: C₂H4(g) + H₂O₂(g)CH₂OHCH₂OH(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

For each of the following unbalanced chemical equations, suppose 1.35 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected (assuming that the limiting reactant is completely consumed). UO₂ (s) + HF (aq) → UF4 (aq) + H₂O(1) a. Limiting reactant: Mass of UF4 = Mass of H₂O = b. Limiting reactant: NaNO3(aq) + H₂SO4 (aq) → Na2SO4 (aq) + HNO3(aq) Mass of Na2SO4 = Mass of HNO3 =

A sample of gas contains 0.1700 mol of N₂(g) and 0.5100 mol of H₂(g) and occupies a volume of 36.9 L. The following reaction takes place: N₂(g) + 3H₂(g) →2NH3(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

The modern periodic table has the elements arranged in order of increasing A. density. B. atomic size . C. atomic weight. D. atomic number. E. charge.

Complete the reaction. Mercuric oxide → + Mercury. Oxide Oxygen Carbon dioxide Nitrogen

What would you multiply "moles of strontium" by to get the units "grams of strontium"?

Exactly 149.0 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C. What is the specific heat capacity of the metal? 0.426 J/g °C 20.7 J/g °C 35.6 J/g °C O2.35 J/g °C None of these choices are correct.

A compound is found to contain 37.32 % phosphorus, 16.88 % nitrogen, and 45.79 % fluorine by mass. The empirical formula for this compound is The molar mass for this compound is 82.98 g/mol. The molecular formula for this compound is

In the laboratory a student finds that it takes 25.3 Joules to increase the temperature of 10.9 grams of gaseous xenon from 23.8 to 39.7 degrees Celsius.

Many metals occur naturally as sulfide compounds; examples include ZnS and CoS. Air pollution often accompanies the processing of these ores, because toxic sulfur dioxide is released as the ore is converted from the sulfide to the oxide by roasting (smelting). For example, consider the unbalanced equation for the roasting reaction for zinc: ZnS (s) + O₂(g) → ZnO(s) + SO2(g) How many kilograms of sulfur dioxide are produced when 240 kg of ZnS is roasted in excess oxygen by this process?

Calculate the work for the expansion of CO₂ from 1.0 to 3.0 liters against a pressure of 1.0 atm at constant temperature. 0 L-atm -2.0 L atm 3.0 L atm 2.0 L atm -3.0 L atm

Given the equation 3A + B → C + D, you react 2 moles of A with 1 mole of B. Which of the following is true? A is the limiting reactant because you need 3 moles of A and have 2. B is the limiting reactant because 3 A molecules react with 1 B molecule. A is the limiting reactant because of its higher molar mass. B is the limiting reactant because you have fewer moles of B than A. Neither reactant is limiting.

Choose the process that requires the most energy when the temperature of 23.4 g ice at -25.0 °C is raised to 37.0 °C. Warming the water Warming the ice to 0.0 °C Melting the ice All of the processes require essentially the same amount of energy.

For the following reaction, 5.21 grams of magnesium nitride are mixed with excess water. The reaction yields 7.00 grams of magnesium hydroxide. magnesium nitride (s) + water (I) → magnesium hydroxide (aq) + ammonia (aq) What is the theoretical yield of magnesium hydroxide? What is the percent yield of magnesium hydroxide?

A sample of solid magnesium is heated with an electrical coil. If 210. Joules of energy are added to a 13.3 gram sample and the final temperature is 37.8°C, what is the initial temperature of the magnesium?

Given the standard enthalpy changes for the following two reactions: (1) Zn(s) + Cl₂(g) → ZnCl₂(s) ΔH°-415.0 kJ (2) Pb(s) + Cl₂(g) → PbCl₂(s) ΔH° -359.4 kJ what is the standard enthalpy change for the reaction: (3) Zn(s) + PbCl₂(s) → ZnCl₂(s) + Pb(s) ΔH° = ?

Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2BrF3(g)- →Br₂(g) + 3F₂(g)

Given the standard enthalpy changes for the following two reactions: (1) 2Fe(s) + O₂(g) →2FeO(s) ΔH = -544.0 kJ (2) Fe(s) + Cl₂(g) →FeCl₂(s) ΔH = -341.8 kJ what is the standard enthalpy change for the reaction: (3) 2FeCl₂(s) + O₂(g)- 2FeO(s) + 2Cl₂(g) ΔH² = ?

A 12.0-g sample of HF is dissolved in water to give 2.0 x 10^2 mL of solution. The concentration of the solution is: 0.06 M 6.0 M 3.0 M 0.12 M 0.60 M

Classify each of the compounds as soluble or not soluble: magnesium sulfate aluminum hydroxide calcium carbonate

A 9.55-g sample of a solid was placed in a 15.00-mL flask. The remaining volume was filled with benzene, in which the solid is insoluble. The solid and benzene together weigh 19.33 g. The density of the benzene is 0.876 g/mL. What is the density of the solid?

Sodium chloride (NaCl) was isolated from SiO₂ and CaCO, by dissolving it in distilled water. Unmentioned is that CaCO, is slightly soluble in water (0.001 g/100 mL). Describe the effect this fact will have on each component of the mixture: will the "isolated" mass of each be greater than, equal to, or less than that in the sample?

Which list represents the classification of the elements nitrogen, neon, magnesium, and silicon, respectively? 1. metal, metalloid, nonmetal, noble gas 2. nonmetal, noble gas, metal, metalloid 3. nonmetal, metalloid, noble gas, metal 4.noble gas, metal, metalloid, nonmetal

On the basis of the element's location in the periodic table, indicate what simple ion each of the following elements is most likely to form. Cl a. Formula of ion: Ra b. Formula of ion: Ca c. Formula of ion:

How many of the following postulates of Dalton's atomic theory are still scientifically accepted? I. All atoms of the same element are identical. II. Compounds are combinations of different atoms. III. A chemical reaction changes the way atoms are grouped together. IV. Atoms are indestructible. 1 0 4 3 2

Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct? No reaction will occur. NH₂SO4 will precipitate from solution. Both KNO3 and NH4SO4 precipitate from solution. A gas is released. KNO3 will precipitate from solution.

What is the energy change when the temperature of 13.3 grams of solid magnesium is decreased from 37.8 °C to 22.3 °C ?

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

Consider the following reaction: CH₂(g) +40₂(g) →CCl₂(g) + 4HCl (g) What mass of CCl4 will be formed if 1.20 moles of methane react with 1.07 moles of chlorine? 41.1 g 658 g 185 g 165 g 19.0 g

The name of an aqueous solution of HF is The formula of hydrochloric acid is