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introductory chemistry atoms first
Introductory Chemistry Atoms First 5th Edition Steve Russo And Michael Silver - Solutions
According to the ideal gas model, why does the chemical identity of a gas not matter when it comes to producing pressure?
A 5.00-L container is filled with 0.8004 g of helium gas at 107.0°C. What is the pressure of the gas in atmospheres and in millimeters of mercury?
A chemical reaction produces 100.0 mL of hydrogen gas at 745.5 mm Hg and 24.0°C. What is the amount of H2 produced in moles and in grams?
What is the density in grams per liter of nitrogen gas at STP?
When it is heated, potassium chlorate decomposes to potassium chloride and oxygen:A sample of solid KClO3 decomposes to produce 150.0 mL of oxygen at 22.0°C and 780.5 mm Hg. How many grams of KClO3 decomposed? 2 KClO3(s) → 2 KCl(s) + 30₂(g)
A gaseous compound of carbon and hydrogen contains 80.0% by mass carbon. A 2.00-L sample has a mass of 2.678 g at STP.(a) Calculate the molar mass of the compound.(b) What is the empirical formula of the compound?(c) What is the molecular formula of the compound?
To what temperature must a gas initially at 20.0°C be heated to double the volume and triple the pressure?
A sample of argon at 0.0°C and 700.0 mm Hg occupies 15.0 mL. What is its volume at STP?
A sample of gas at 25.0°C and 655 mm Hg has a density of 2.26 × 10–3 g/mL. What is the molar mass of the compound?
In the Haber process, nitrogen reacts with hydrogen to produce ammonia: N2(g) + 3H2(g) → 2NH3(g)(a) Suppose 2.0 L of N2 gas at STP is combined with 6.0 L of H2 gas, with the two gases being at the same temperature and pressure.Is this reaction being run in a balanced fashion or in a limiting
How many atoms of nitrogen are there in a 230.0-mL sample of N2O4 gas that has a pressure of 745.0 mm Hg at 34.0°C?
A sample of gas at 25°C and 759.0 mm Hg has a volume of 1.58L. If the temperature is raised to 35°C but the pressure is held constant at 759.0 mm Hg, will the volume increase or decrease? Explain your answer.
Consider two identical 1-L containers, both at room temperature (300 K). One of them contains 1 mole of helium gas, and the other contains 1 mole of hydrogen gas. Is the pressure higher in the helium container, higher in the hydrogen container, or the same in the two containers?
Consider two identical 1-L containers, both at room temperature (300 K). One of them contains 1.0 g of helium gas, and the other contains 1.0 g of hydrogen gas. Is the pressure higher in the helium container, higher in the hydrogen container, or the same in the two containers?
What volume in milliliters of N2O4 gas at 0.996 atm and 25.0 °C contains 0.200 g of oxygen?
Carbon dioxide in a gas cylinder of unchangeable volume is at a pressure of 25.0 atm at 25°C. When placed in the sunlight on a hot summer day, the temperature increases to 40°C. What is the new pressure of the CO2?
When a balloon is placed in a freezer, the size of the balloon decreases. Explain why.
A sample of Ne gas in a 10.0-L container at 25.0 °C exerts a pressure of 7.35 atm. What is the number of moles of Ne in the container? What is the mass in grams of the Ne?
Of the values for P, V, n, and T, which ones remain constant during the following changes?(a) Air in a sealed glass bulb is heated from 25°C to 32°C.(b) An He-filled balloon is cooled from 23°C to 10°C.(c) The amount of CO2 in a sealed steel cylinder is increased by adding 50.0 g of CO2.
Under what two conditions are gas molecules unable to overcome the weak attractive forces that exist between them?
Arrange these gases, all at STP, in order of increasing density: CO2, H2, O2, CH4, He.
If a gas sample occupies 1.80 L at 250 °C and 792 mm Hg, what is the number of moles in the sample?
Which variable is not needed to describe the behavior of an ideal gas: volume, number of moles, temperature, molar mass, or pressure?
(a) How many liters of O2 are there in 5.38 moles at STP?(b) How many moles of NH3 are there in 859 mL at STP?(c) How many moles of H2 are there in 0.518 L at STP?
Are gases denser or less dense than liquids and solids? Explain.
If a gas occupies 2.40 L at 1 atm and 22 °C, at what Celsius temperature will it occupy 7.20 L at 1 atm?
A chemistry student realizes she has forgotten the value of R and needs to determine it experimentally. She decides to measure the mass, volume, pressure, and temperature of a sample of carbon dioxide gas. She finds that 4.505 g of the gas occupies 2.50 L at 23 °C and 0.9960 atm. Calculate the
A gas at 25.0 °C occupies a volume of 5.00 gallons and exerts a pressure of 755 mm Hg. Express (a) The temperature of the gas in Kelvin, (b) The volume of the gas in liters, (c) The pressure of the gas in atmospheres.
In the ideal gas law, pressure must be expressed in units of ______, volume must be expressed in units of ______, temperature must be expressed in ______, and n represents the number of ______.
A radial tire has an air pressure of 2.20 atm at 32°F. After hours of high-speed driving, the temperature of the air in the tire reaches 80°F. What is the pressure in the tire at this temperature? Assume that the volume of the tire does not change.
An 84.0-g sample of an unknown gas occupies 60.8 L at 23 °C and 1.2 atm. What is the molar mass of the gas?
True or false? In order to determine the volume occupied by 3.0 moles of an ideal gas at 28°C and 1.4 atm, the identity of the gas must be known. If the statement is false, explain why.
What is the density of He gas in a cylinder if the pressure of the gas is 15.2 atm and its temperature is 22°C?
In an ideal gas, the molecules are considered to have no _____ forces.
In the laboratory preparation of oxygen gas, the following reaction is carried out: 2KClO3(s) → 2KCl(s) + 3O2(g)(a) How many moles of oxygen gas can be produced from the decomposition of 500.0 g of KClO3?(b) What volume in liters would the oxygen gas produced in part (a) occupy at 24.0 °C and
(a) If the temperature of a gas is doubled while the pressure is kept constant, the volume of the gas _____.(b) If the pressure of a gas is halved while the temperature is kept constant, the volume of the gas _____.
What is the Celsius temperature of a gas if 3.200 moles of it occupy 12.00 L at 8.500 atm?
A 1.25-g sample of a gas of unknown identity occupies 2.50 L and exerts a pressure of 0.400 atm at 0 °C.(a) What is the molar mass of the gas?(b) Combustion analysis determines that the empirical formula of the gas is CH2. What is its molecular formula?
If a quantity of gas occupies 850 mL at 300 K and 750 mm Hg, what volume in milliliters will the gas occupy at 200 K and 1200 mm Hg?
Perform the following conversions:(a) 30.2 in. Hg to millimeters of mercury(b) 890.0 mm Hg to atmospheres(c) 300.0 lb/in.2 to atmospheres
If 8.50 moles of He gas occupy a volume of 25.0 L at 28°C, what pressure in atmospheres does the gas exert?
If 48.3 g of an unknown gas occupies 10.0 L at 40°C and 3.10 atm, what is the molar mass of the gas?
A gas tank contains CO2 at a pressure of 6.80 atm. What would the CO2 pressure be if the container were (a) Twice as large and(b) One-fourth as large?
What is the molar mass of a gas whose density is 1.52 g/L at 0°C and 1 atm pressure?
Explain why gases always occupy the entire container they are in, but solids and liquids do not.
Consider the following two plots:(a) Which of the two plots represents an inverse relationship? Express the inverse relationship in an English statement.(b) A student looks at the plot and declares that grades are proportional to 1/hours of TV. Is he correct? Explain why.(c) A student looks at the
What happens to the volume of a gas in a cylinder with a movable piston if:(a) The pressure is doubled while the temperature is held constant?(b) The temperature is doubled while the pressure is held constant?(c) The pressure and the temperature are both doubled?(The movable piston means the volume
Something is done to this tank of gas to make the pressure change as shown.Give at least two different ways this could have been accomplished. P = 10 atm P = 20 atm
Consider two balloons, both in the same room and both exactly the same volume. Consider also the balanced reaction between these gases.If we allow the gases from these balloons to mix and react, will there be a limiting reactant? If so, which is it, and how did you know? H₂ 2H₂ + O₂ 2H₂O
If we continuously compress a real gas in a cylinder with a movable piston while keeping the container at a constant temperature in an ice bath:(a) What will eventually happen to the gas and why?(b) How well will the ideal gas law apply to the real gas shown when it is close to doing what you said
You are trapped on a desert island without any reference books, and you need the value of the ideal gas constant R. Luckily, you stumble upon the following tank of helium (see below). Use what you found to calculate the value of R. Make sure your units are L · atm/K · mol. Oh, by the way, while
Real gases are not ideal gases. Explain why this is so in terms of intermolecular forces, and then describe (and justify) what conditions with regard to temperature and pressure will bring a real gas close to behaving like an ideal gas.
Consider three identical-sized cylinders, all at the same temperature. Cylinder A contains 2 moles of nitrogen (N2) gas. Cylinder B contains 1 mole of nitrogen gas and 1 mole of methane (CH4) gas. Cylinder C contains 2 moles of methane gas. Which cylinder has the higher pressure?
Suppose the pressure in cylinder A in the previous problem was 2.50 atm. What do you think the pressure due to methane is in cylinder B? Justify your answer with some sort of explanation. Then Google “Dalton’s Law” and explain how it relates to this problem.Data from Previous problemConsider
Normal atmospheric pressure will push a column of mercury up an evacuated glass tube (a barometer) to a height of 76 cm (760 mm Hg), which we call one atmosphere. Suppose water were used as the liquid in a barometer instead of mercury. How high up would the atmosphere push a column of water in
Normal atmospheric pressure is 1 atm = 760 mm Hg. However, it is also 14.7 lbs/in.2 (14.7 pounds per square inch). Given that liquid mercury has a density of 13.6 g/mL, explain (show a calculation) why 1 atm also equals 14.7 lbs/in.2. Then, go back to the introduction of this chapter and calculate
You are on the balcony of the upper floor of a high-rise building in Chicago. Way down below on the street, your friend is engaged in conversation with someone and is drinking a particularly flavorful mixed drink. You decide to take a sip from his glass without his knowing, so you collect together
Consider a container that contains 1.00 mole of CO2(g) at 298K.(a) What does the ideal gas law predict the pressure to be in atm?(b) What does the van der Waals equation predict the pressure to be?(c) What is the percent difference of the van der Waals pressure from the ideal pressure?(d) Suppose
In an aqueous solution of sugar:(a) Sugar is the solvent and water is the solute.(b) Water is the solvent and sugar is the solute.(c) There is no solvent because aqueous means water.(d) The composition of the solution is nonhomogeneous.
Classify the following as solutions or heterogeneous mixtures:(a) A hot cup of instant coffee(b) Chicken vegetable soup(c) Unfiltered blood(d) Filtered blood plasma(e) A chromium-plated steel automobile bumper(f) A stainless steel automobile bumper (stainless steel is prepared by combining iron,
Water bugs can walk on the surface of the water in a swimming pool, but if you add a little soap, they no longer can (they fall through). Why do you think this is so?
From what you learned about the different phases of matter, why do you think it is necessary to employ the liquid or gas phase to obtain the homogeneity needed to form a solution?
A finely ground mixture of solid sugar with solid salt is:(a) A heterogeneous mixture.(b) A homogeneous mixture.(c) A solution.(d) A nonaqueous solution.
Identify the solvent and solute or solutes in each solution:(a) Nail-polish remover (30% acetone in water)(b) Humid air(c) Stainless steel(d) Aqueous solution of aspirin
Suppose you want to make a 1 M ethanol solution in water (ethanol is a clear, colorless liquid). What is wrong with adding 1 mole of ethanol to 1 liter of water to make this solution? What wrong assumption is involved in doing this?
In order for a solute to dissolve in a solvent, there must be:(a) Ion-dipole forces between solvent molecules.(b) Repulsion between solvent and solute molecules.(c) Intermolecular attraction between solvent and solute molecules.(d) Weak intermolecular forces between solute molecules.
The “proof” value of any liquor is equal to twice the percentage of alcohol; for example, a 50-proof liquor is 25% alcohol in water. Vodka is normally sold between 80 and 100 proof, but suppose you came across a bottle of 135-proof vodka. Would you be justified in calling the alcohol the
For the (attempted) dissolution of NaCl in carbon tetrachloride, CCl4, choose the best answer for the energy required in each step.
Solvation is a step in the dissolving process that:(a) Always takes some energy.(b) Always releases some energy.(c) Is independent of any energy changes.(d) Has little to do with whether or not a solution will form.
Consider the ionic compound magnesium chloride, MgCl2. Do you think the hydration energy for this compound is greater than, less than, or about equal to that of NaCl?
An H-shaped tank contains gas A in one arm and gas B in the other arm. When a valve separating the two arms is opened, the gases will spontaneously mix if given enough time. The reverse process—the gases spontaneously separating into all A in one arm and all B in the other—will never happen, no
For a solute to dissolve in a solvent, it is best that:(a) Solvation requires more energy than solvent separation and solute separation.(b) Solvation releases as little energy as possible.(c) The sum of the energy required for solute and solvent separation be huge.(d) Solvation releases more energy
Imagine you are trying to dissolve NaCl in liquid carbon tetrachloride, CCl4. Would the energy released in the solvation step be greater than, less than, or about equal to that released when NaCl dissolves in water? Explain.
The density of ethanol is 0.7893 g/mL. Use this information to determine the number of grams of ethanol in the 79.6 mL of 30.0 vol % solution just discussed.
With respect to entropy, when a solution forms:(a) Entropy increases.(b) Solute particles become more randomized.(c) We obtain a more probable distribution of solute particles.(d) The increase in entropy can sometimes overcome a positive ΔEtotal for dissolving.(e) (a), (b), (c), and (d) are
Based on the answer to Practice Problem 12.4, is the energy required for solute separation greater for NaCl or MgCl2? Explain.Data from Problem 12.4Consider the ionic compound magnesium chloride, MgCl2. Do you think the hydration energy for this compound is greater than, less than, or about equal
A saturated solution is a solution:(a) Where the concentration of solute is at a maximum.(b) Where the molarity is greater than the maximum possible.(c) Prepared by using excess solvent to dissolve the solute.(d) Where the concentration is given in terms of moles of solute per liter of solution.
On the basis of the three steps involved in the formation of a solution, what is the biggest difference between dissolving a gas and dissolving a solid?
How many milliliters of a 1.500 M solution of NaCl do you need to obtain 100.0 g of NaCl?
How many milliliters of a 2.55 M solution of glucose, C6H12O6, molar mass = 180.155 g/mol, do you need to obtain 25.0 g of glucose?
How many grams of ethanol, C2H6O, are there in 200.0 mL of a 2.00 M aqueous solution of ethanol?
Come up with five things from everyday life for which you can determine a rate. For each, express what the usual rate (or range of rates) is in appropriate units.
Give a third reason a single-step mechanism of product formation is unlikely. (Focus on the products. The reaction of methane and oxygen produces CO2 and H2O. There are certainly many other possible combinations of carbon, hydrogen, and oxygen, however, such as CH2O (formaldehyde), CO (carbon
Consider this reaction-energy profile for the reaction A → B:(a) Is this reaction exothermic or endothermic?(b) Will the container in which this reaction is carried out feel hot or cold to the touch? Explain.(c) What is the value of ΔErxn (include the sign)?(d) What does the sign of ΔErxn tell
Kinetics is the study of:(a) The rates of chemical reactions (how fast or slow they go and things that effect this).(b) The stoichiometry of chemical reactions (how much reactants they consume or products they form).(c) How much energy a reaction releases or consumes as reactants turn into
Here is the reaction-energy profile from Practice Problem 13.1 for the exothermic reaction A S B, for which ΔErxn = –40 kj/mol. What is ΔErxn for the reverse reaction A ← B?Data from Problem 13.1Consider this reaction-energy profile for the reaction A → B:Is this reaction exothermic or
Some reactions have rate laws that include a product concentration raised to the –1 order. An example of that is the hypothetical reaction A + B + E → D + F where the rate law is: Rate = k[A][B][E][D]–1This can also be written equivalently as: Rate = k[A][B][E]/[D]What effect does an increase
Kinetics studies are often performed for the following reason:(a) To determine the purity of the products of the reaction.(b) To give insight into the mechanism of the reaction (how it occurs at the molecular level).(c) To give insight into the electronegativities of the reactant atoms.(d) To help
Here are data for three hypothetical reactions:For each reaction, (a) Sketch the reaction-energy profile.(b) Indicate whether the reaction is endothermic or exothermic.(c) Determine the value of ΔErxn.(d) Determine the value of Ea. Energy of Energy of Reaction reactants (kJ/mol) products
A reaction is endothermic by 65 kJ/mol (that is, ΔErxn = +65 kJ for every mole of product formed).(a) Draw a reaction-energy profile for this reaction, assuming the energy of the reactants to be 100 kJ/mol.(b) Does this reaction go uphill or downhill in energy?(c) What is the value of ΔErxn?(d)
A reaction that is exothermic:(a) Has its products at a lower energy than its reactants.(b) Has a negative ΔErxn.(c) Can be said to go downhill in energy.(d) All of the above are correct.
In Equation 13.1 (repeated on next page), which factor or factors do you think a catalyst would alter?Equation 13.1 Number of collisions per Fraction of collisions in which Reaction rate = unit time with energy equal X molecules have proper orientation to or greater than Ea Energy
A reaction has a ΔErxn of –450 kJ/mol. The products have an energy of 20 kJ/mol.(a) Is the energy of the reactants higher or lower than that of the products? Explain.(b) What is the energy of the reactants?(c) Is the reaction exothermic or endothermic? How do you know?(d) Does the reaction go
In order for bonds within reactants to break during a chemical reaction:(a) Energy is sometimes required and sometimes released (depends on ΔErxn).(b) Energy is required, always!(c) Energy is released.(d) Bonds break spontaneously without the involvement of energy.
The energy released by the reaction A → B is 400 kJ/mol.(a) What is ΔEforward rxn? (b) What is ΔEreverse rxn?
Suppose a reaction has a large k value.(a) What does this say about Ea for the reaction?(b) What does this say about the orientation requirements of the reaction?(c) Is such a reaction intrinsically fast or slow?
Why should the number of collisions per second between reactant molecules have anything to do with their concentration?
Suppose the rate did not change when we ran experiments 1 and 3 in Table 13.1. Write the rate law. What is the overall order of the reaction? Table 13.1 Rate Data for Reaction 13.9 at 904 °C Experiment 1 2 3 Initial concentration of NO (mol/L) 0.210 0.210 0.420 Initial concentration of H₂
Judging from the following reaction-energy profile, is the reaction endothermic or exothermic? What is the value of ΔErxn? 240 kJ/mol Energy 190 kJ/mol Reactants Start Products Finish Reaction coordinate
According to the reaction-energy profile in Problem 13.44, the products are higher in energy than the reactants. What must occur during the course of the reaction for this to occur?Data from Problem 13.44Judging from the following reaction-energy profile, is the reaction endothermic or exothermic?
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