A gas has an initial pressure of 1.445 atm and an initial volume of 1.009 L. What is its new pressure if volume is changed to 0.556 L? Assume temperature and amount are held constant.

A gas has an initial pressure of 633 torr and an initial volume of 87.3 mL. What is its new pressure if volume is changed to 45.0 mL? Assume temperature and amount are held constant.

A sample of gas doubles its pressure and doubles its absolute temperature. By what amount does the volume change?

Use Gay-Lussacs law to determine the final temperature of a gas whose initial pressure is 1.88 atm, initial temperature is 76.3 K, and final pressure is 6.29 atm. Assume volume and amount are held...

What is the density of SF6 at 335 K and 788 torr?

A sample of gas has a volume of 3.91 L, a temperature of 305 K, and a pressure of 2.09 atm. How many moles of gas are present?

A 3.88 mol sample of gas has a temperature of 28C and a pressure of 885 torr. What is its volume?

A sample of 87.4 g of Cl2 has a temperature of 22C and a pressure of 993 torr. What is its volume in milliliters?

A sample of NO2 is collected over water in a 775 mL container at 25C. If the total pressure is 0.990 atm, how many moles of NO2 are collected?

In a gas mixture of O2 and N2, the total pressure is 2.66 atm and the partial pressure of O2 is 888 torr. What is the partial pressure of N2?

A sample of O2 is collected over water in a 5.00 L container at 20C. If the total pressure is 688 torr, how many moles of O2 are collected?

Use two values of R to determine how many joules are in a liter atmosphere.

At an altitude of 40 km above the earths surface, the atmospheric pressure is 5.00 torr, and the surrounding temperature is 20(C. If a weather balloon is filled with 1.000 mol of Heat 760 torr and...

NaHCO3 is decomposed by heat according to If you start with 100.0 g of NaHCO3 and collect 10.06 L of CO2 over water at 20C and 0.977 atm, what is the percent yield of the decomposition reaction?...

What is the pressure in pascals if a force of 3.44104 MN is pressed against an area of 1.09 km2?

What is the final pressure of a gas whose initial conditions are 1.407 L, 2.06 atm, and 67C and whose final volume and temperature are 608 mL and 449 K, respectively? Assume the amount remains...

A sample of 6.022 1023 particles of gas has a volume of 22.4 L at 0(C and a pressure of 1.000 atm. Although it may seem silly to contemplate, what volume would 1 particle of gas occupy?

One mole of liquid N2 has a volume of 34.65 mL at 196(C. At that temperature, 1 mol of N2 gas has a volume of 6.318 L if the pressure is 1.000 atm. What pressure is needed to compress the N2 gas to...

An experimenter adds 336 J of heat to a 56.2 g sample of Hg. What is its change in temperature? The heat capacity of Hg is in Table 7.1.

An unknown mass of Al absorbs 187.9 J of heat and increases its temperature from 23.5(C to 35.6(C. What is the mass of the aluminum? How many moles of aluminum is this?

To warm 400.0 g of H2O, 0.050 mol of ethanol (C2H5OH) is burned. The water warms from 24.6(C to 65.6(C. What is the heat of the reaction, and what is the H of the reaction on a molar basis?

Given the thermochemical equation 2Na+(aq) + SO42(aq) ( Na2SO4(s)H = 819.8 kJ How much energy is absorbed when 55.9 g of Na+(aq) are reacted?

Determine H for the reaction Fe2(SO4)3 ( Fe2O3 + 3SO3 Given these data: 4Fe + 3O2 ( 2Fe2O3 H = 1,650 kJ 2S + 3O2 ( 2SO3 H = 792 kJ 2Fe + 3S + 6O2 ( Fe2(SO4)3 H = 2,583 kJ

The basic reaction in the refining of aluminum is to take Al2O3(s) and turn it into Al(s) and O2(g). Write the balanced thermochemical equation for this process.

What is the heat when 1,744 g of Hg increase in temperature by 334(C? Express your final answer in kJ.

What is the heat when 13.66 kg of Fe cool by 622(C? Express your final answer in kJ.

What is final temperature when 967 g of Au at 557(C lose 559 J of heat?

What is the energy of a photon if its frequency is 2.06 1018 s1?

What is the frequency of light if its wavelength is 1.226 m?

What is the frequency of light if its wavelength is 733 nm?

What is the wavelength of light if its frequency is 1.009 106 Hz?

Write the abbreviated electron configuration for each atom in Exercise 8. In exercise 8 Write the complete electron configuration for each atom. a. Br, 35 electrons b. Be, 4 electrons

Write the abbreviated electron configuration for each atom in Exercise 9. In exercise 9 Write the complete electron configuration for each atom. a. Cd, 48 electrons b. Mg, 12 electrons

A third-row element has the following successive IEs: 1,012, 1,903, 2,912, 4,940, 6,270, and 21,300 kJ/mol. Identify the element.

a. Predict the electron configurations of Ga through Kr. b. From a source of actual electron configurations, determine how many exceptions there are from your predictions in part a.

Bi (atomic number 83) is used in some stomach discomfort relievers. Using its place on the periodic table, predict its valence shell electron configuration.

How many IEs does a Be atom have? Write the chemical reactions for the successive ionizations.

Domestic microwave ovens use microwaves that have a wavelength of 122 mm. What is the energy of one photon of this microwave?

Draw the Lewis electron dot diagram for each ion. a. In+ b. Br

How many electrons does an N atom have to gain to have a complete octet in its valence shell?

Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed. a. CN b. C2Cl2 (assume two central atoms)

Identify the electron group geometry and the molecular geometry of each molecule. a. CS2 b. H2S

Which bond do you expect to be more polaran OF bond or an SO bond?

Use bond energies to estimate the energy change of this reaction. N2H4 + O2 ( N2 + 2H2O

Identify the strongest intermolecular force present in each substance. a. He b. CHCl3 c. HOF

The Hsub of I2 is 60.46 kJ/mol, while its Hvap is 41.71 kJ/mol. What is the Hfus of I2?

What is the energy change when 30.8 g of Al solidify at 660C?

What is the energy change when 111 g of Br2 boil at 59.5C?

What is the energy change when 98.6 g of H2O condense at 100C?

Predict the type of solid exhibited by each substance. a. BN (boron nitride, a diamond-like compound) b. B2O3 c. NaBF4

Explain how the bonding in an ionic solid explains some of the properties of these solids.

What is the mass percentage of H2O2 in a solution with 1.67 g of H2O2 in a 55.5 g sample?

Which solvent is NaOH more likely soluble inCH3OH or C6H6?

What volume of 1.772 M BaCl2 is needed to obtain 123 g of BaCl2?

Differentiate between mass percentage and parts per thousand.

How much water must be added to 1.55 L of 1.65 M Sc(NO3)3(aq) to reduce its concentration to 1.00 M?

If 12.00 L of a 6.00 M HNO3 solution needs to be diluted to 0.750 M, what will be its final volume?

If 665 mL of a 0.875 M KBr solution are boiled gently to concentrate the solute to 1.45 M, what will be its final volume?

If 1.00 L of an LiOH solution is boiled down to 164 mL and its initial concentration is 0.00555 M, what is its final concentration?

How much water must be added to 75.0 mL of 0.332 M FeCl3(aq) to reduce its concentration to 0.250 M?

What volume of 0.779 M NaCl will react with 40.8 mol of Pb(NO3)2? Pb(NO3)2 + 2NaCl ( PbCl2 + 2NaNO3

It takes 4.667 mL of 0.0997 M HNO3 to dissolve some solid Cu. What mass of Cu can be dissolved? Cu + 4HNO3(aq) ( Cu(NO3)2(aq) + 2NO2 + 2H2O

It takes 49.08 mL of 0.877 M NH3 to dissolve some solid AgCl. What mass of AgCl can be dissolved? AgCl(s) + 4NH3(aq) ( Ag(NH3)4Cl(aq)

What mass of 3.00% H2O2 is needed to produce 66.3 g of O2(g)? 2H2O2(aq) ( 2H2O() + O2(g)

A 0.75% solution of Na2CO3 is used to precipitate Ca2+ ions from solution. What mass of solution is needed to precipitate 40.7 L of solution with a concentration of 0.0225 M Ca2+(aq)? Na2CO3(aq) +...

Using concentration as a conversion factor, how many liters are needed to provide 2.500 mol of (NH2)2CO from a 1.087 M solution?

What is the mass of solute in 24.5 mL of 0.755 M CoCl2?

What volume of solution is needed to provide 9.04 g of NiF2 from a 0.332 M solution?

What volume of solution is needed to provide 0.229 g of CH2O from a 0.00560 M solution?

At 300C, the vapor pressure of Hg is 32.97 torr. What mass of Au would have to be dissolved in 5.00 g of Hg to lower its vapor pressure to 25.00 torr?

If 125 g of N2 are mixed with 175 g of O2, what is the mole fraction of each component?

An alloy of stainless steel is prepared from 75.4 g of Fe, 12.6 g of Cr, and 10.8 g of C. What is the mole fraction of each component?

A solution is made by mixing 12.0 g of C10H8 in 45.0 g of C6H6. If the vapor pressure of pure C6H6 is 76.5 torr at a particular temperature, what is the vapor pressure of the solution at the same...

A solution is made by mixing 43.9 g of C6H12O6 in 100.0 g of H2O. If the vapor pressure of pure water is 26.5 torr at a particular temperature, what is the vapor pressure of the solution at the same...

What volume of 12.0 M HCl solution is needed to obtain exactly 1.000 kg of HCl?

Write the balanced chemical equation for the neutralization reaction between Sr(OH)2 and H3PO4. What is the salt?

Predict the products of this reaction, assuming it undergoes a Brnsted-Lowry acid-base reaction. (C2H5)3N + H2O ( ?

The methoxide ion (CH3O) acts as a Brnsted-Lowry base in water. Write the hydrolysis reaction for the methoxide ion and identify the Brnsted-Lowry acid and Brnsted-Lowry base.

Identify the Brnsted-Lowry acid and Brnsted-Lowry base in this chemical equation. H2C2O4 + 2F ( 2HF + C2O42

If 16.33 mL of 0.6664 M KOH was needed to titrate a sample of HC2H3O2 to its equivalence point, what mass of HC2H3O2 was present?

Identify each salt as neutral, acidic, or basic. a. NH4I b. C2H5NH3Cl c. KI

Identify each salt as neutral, acidic, or basic. a. KC2H3O2 b. KHSO4 c. KClO3

Write a chemical equation for the ionization of each base and indicate whether it proceeds 100% to products or not. a. NH3 b. (CH3)3N c. Mg(OH)2

For a given aqueous solution, if [OH] = 1.0 1012 M, what is [H+]?

For a given aqueous solution, if [H+] = 1.0 109 M, what is [OH]?

What is the pH of a solution when [OH] is 0.0222 M?

Which combinations of compounds can make a buffer? Assume aqueous solutions. a. H3PO4 and Na3PO4 b. NaHCO3 and Na2CO3 c. NaNO3 and Ca(NO3)2 d. HN3 and NH3

The following reaction is at equilibrium: PBr3 + Br2 + PBr5 The equilibrium [Br2] and [PBr5] are 2.05 M and 0.55 M, respectively. If the Keq is 1.65, what is the equilibrium [PBr3]?

Given this equilibrium, predict the direction of shift for each stress. H2(g) + F2(g) + 2HF (g) + 546 kJ a. Increased temperature b. Addition of H2 c. Decreased pressure

Given this equilibrium, predict the direction of shift for each stress listed. Co2(g) + C(s) + 171kJ + 2CO (g) a. Addition of CO b. Increased pressure c. Addition of a catalyst

Assign oxidation numbers to the atoms in each substance. a. PCl5 b. (NH4)2Se c. Ag d. Li2O2

Assign oxidation numbers to the atoms in each substance. a. C6H6 b. B(OH)3 c. Li2S d. Au

A voltaic cell is based on this reaction: 3Pb + 2V3+ ( 3Pb2+ + 2V If the voltage of the cell is 0.72 V, what is the standard reduction potential of the V3+ + 3e ( V half reaction?

Name each molecule. a. b. C

Identify each compound as a primary, secondary, or tertiary amine. a. b. c. NH HIN NH2 NH2

Draw the polymer made from this monomer. H C2H5

Draw the carbon backbone of all possible five-carbon cyclic alkenes with two double bonds, assuming no substituents on the ring.

Draw the structure of the final product of the double elimination of 1,3-dibromopropane.

A 33.0-g sample of an unknown liquid at 20.0oC is heated to120oC. During this heating, the density of the liquid changes from 0.854 g/cm3 to 0.797 g/cm3. What volume would this sample occupy at 120oC?

A solution is prepared by dissolving table salt, sodium chloride, in water at room temperature. a. Assuming there is no significant change in the volume of water during the preparation of the...