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introductory chemistry atoms first

Questions and Answers of Introductory Chemistry Atoms First

Propane reacts with oxygen to produce CO2 and H2O, as shown in the balanced equation:Write this reaction in words using the word mole(s) four times. C3H8 +50₂ 3 CO₂ + 4H₂O
How many moles of carbon atoms are there in 2 moles of propane?
It is possible to go from a molecular formula to percent by mass composition for each element because (a) The formula subscripts can be interpreted as grams of each element present.(b) The formula
Suppose you have 100.0 g of H2O.(a) How many moles of H2O molecules do you have?(b) How many H2O molecules do you have?
Suppose you have 0.565 moles of HI.(a) How many grams of HI do you have?(b) How many HI molecules do you have?
(a) Balance this unbalanced equation by inspection:(b) Express this reaction in words, using the word mole(s) wherever appropriate.(c) To produce 1 mole of C6H12 from this reaction, how many grams of
Suppose you have 5.000 × 1024 molecules of methane, CH4.(a) How many moles of methane do you have?(b) How many grams of methane do you have?
(a) Express the balanced chemical equation CH4 + 2O2 → 2 H2O + CO2 in words, using the word mole(s) wherever appropriate.(b) To produce 1 mole of CO2 from this reaction, how many grams of CH4 and
(a) Balance this unbalanced equation by inspection:(b) Express this reaction in words, using the word mole(s) wherever appropriate.(c) To produce 6 moles of H2O from this reaction, how many grams of
How many grams of oxygen does it take to burn 10.0 g of glucose?
How many grams of water will be produced by burning 10.0 g of glucose?
What is the theoretical yield in grams of carbon dioxide if 10.0 g of glucose is burned?
If 10.0 g of carbon dioxide was produced, how many grams of glucose must havebeen burned?
How many O atoms are there in 10.7 g of oxygen, O2, molecules?
How many aluminum atoms are there in 10.0 g of aluminum oxide, Al2O3?
How many molecules of water are there in 10.0 g of water?
What do we mean by the theoretical yield of a reaction?
Consider a sample of 24.0 g of O2 molecules.(a) How many moles of O2 molecules are present?(b) How many moles of O atoms are present?
How many grams of glucose (C6H12O6) would you need to get 5.00 × 1030 carbon atoms?
Consider the unbalanced chemical equation CaC2 + CO → C + CaCO3When the reaction is complete, 135.4 g of CaCO3 is produced and 38.5 g of CaC2 is left over. Assuming the reaction had a 100% yield,
Consider the unbalanced chemical equation N2O4 + N2H4 → N2 + H2O(a) Balance the equation.(b) If 42.32 g of N2 was produced and the reaction yield was 67.5%, how many grams of N2O4 and N2H4 were
Use the method of dividing moles by coefficients to determine whether the reaction is being run in a balanced or limiting fashion. If it is being run in a limiting fashion and you are asked for
Use the method of dividing moles by coefficients to determine whether the reaction is being run in a balanced or limiting fashion. If it is being run in a limiting fashion and you are asked for
Use the method of dividing moles by coefficients to determine whether the reaction is being run in a balanced or limiting fashion. If it is being run in a limiting fashion and you are asked for
A compound is known to contain carbon and hydrogen. It might also contain oxygen. A sample of the compound is burned. The results of the combustion analysis are 74.9% C and 25.1% H.(a) What is the
A compound is found to contain 52.4% carbon and 13.1% hydrogen. It might also contain oxygen.(a) What is the chemical formula for this compound?(b) Write the balanced combustion reaction (reaction
A compound is known to contain carbon and hydrogen and might also contain oxygen. A sample is burned yielding 54.6% C and 9.16% H.(a) What is the empirical formula of the compound?(b) The molar mass
A compound is known to contain carbon and hydrogen and might also contain oxygen. A sample is burned yielding 85.62% C and 14.37% H. (Be careful here. Remember, there is always a little inaccuracy
What is the mass percent of each element in hydrogen peroxide, H2O2?
What is the mass percent of each element in trinitrotoluene (TNT), C7H5N3O6?
A compound is found to have the following elemental mass percents: Cl = 89.09%, C = 10.06%, H = 0.84%. The molar mass of the compound is 119.378 g/mol. What are the empirical and molecular formulas?
A compound is known to contain C and H, and might also contain O. It is analyzed for C and H only, yielding the mass percents C = 54.53% and H = 9.15%. The molar mass of the compound is 88.106 g/mol.
How is a balanced chemical equation like a recipe?
Consider this recipe for 1 dozen cookies:(a) Write at least five conversion factors that might be useful for solving cookie stoichiometry problems.(b) Using unit analysis, calculate how many cups of
One recipe for cheesecake is the following, which makes one cake:(a) To bake three cakes, how many eggs do you need? Write down your method and cross out units that cancel.(b) If you have 63 blocks
How is the concept of “1 mole” similar to the concept of “1 dozen”?
When is it allowed to insert the word mole into a chemical equation when translating the equation into words?
The human population of our planet is about 6 billion people. What percentage of a mole is 6 billion?
Consider bicycles where each wheel has 24 spokes.(a) How many bicycles are there in 1 mole of bicycles?(b) How many tires are there in 1 mole of bicycles?(c) How many spokes are there in 1 mole of
How many O2 molecules are there in 1 mole of O2 molecules? How many O atoms are there in 1 mole of O2 molecules?
How many pennies are there in 2.5 moles of pennies? How many dollars does this equal? Answer both questions by using conversion factors, and show which units cancel.
How many years are there in 1 mole of seconds? Use conversion factors, and show which units cancel.
Sometimes using the word moles when translating a chemical equation into words can be very helpful. For example, consider the following correctly balanced equation. What difficulty do you run into
Translate the following balanced equation into words, first without using the word moles, then again with the word moles:2 SO2 + O2 → 2 SO3
In words, what is the mass of 1 mole of atoms of any element?
In words, what is the mass of 1 mole of any molecule?
How do you calculate the molar mass of a compound?
How does molar mass solve the “language problem” when a chemical equation is being used as a recipe?
How many atoms of the 126C isotope are there in exactly 12 g of the isotope?
Consider a sample containing 12.011 g of naturally occurring carbon.(a) How many carbon atoms are in this sample?(b) How many dozens of carbon atoms are in this sample?(c) How many moles of carbon
If you have 1 mole of glucose (C6H12O6):(a) How many moles of carbon atoms do you have?(b) How many moles of hydrogen atoms do you have?(c) How many oxygen atoms do you have?(Note that we are not
Consider the ammonia (NH3) molecule.(a) If you have 1 mole of ammonia, how many moles of H atoms do you have?(b) If you have 2 moles of ammonia, how many moles of H atoms do you have?(c) If you have
What do we mean by the actual yield of a reaction?
Why is the actual yield of a reaction often not equal to the theoretical yield?
What do we mean by the percent yield of a reaction?
A student runs a reaction to prepare 40.0 g of aspirin and yet recovers only 15.5 g. What is the percent yield?
Consider the unbalanced chemical equation NO + O2 → NO2(a) Balance the equation.(b) Translate the equation into words using the word mole(s) wherever you can.(c) To produce 2 moles of NO2 by the
Consider the unbalanced chemical equation HCl + Zn → H2 + ZnCl2 (a) Balance the equation.(b) Translate the equation into words using the word mole(s) wherever you can.(c) To produce 1 mole of H2
Consider the unbalanced chemical equation Na + Cl2 → NaCl(a) Balance the equation.(b) Translate the equation into words using the word mole(s) wherever you can.(c) To produce 1 mole of NaCl from
The formula C6H12O6 is a source of many conversion factors.(a) Write at least three of them.(b) Suppose you have a sample of C6H12O6, and it contains a total of 72,000 hydrogen atoms. How many carbon
The balanced chemical equation 2 AgBr → 2 Ag + Br2 and the formulas of the substances in it are a source of many conversion factors. Write all that are possible using the word mole(s).
The following chemical equation is unbalanced:I2 + Cl2 → ICl3 (a) Balance the equation.(b) The balanced equation is a source of many conversion factors containing the two reactants and one
How many H atoms are there in 2.0158 g of H atoms?
Consider a sample of 92.5 g of O2 molecules.(a) How many moles of O2 molecules are present?(b) How many moles of O atoms are present?(c) How many O atoms are present, and how much larger should this
Consider sulfuric acid, H2SO4, used in car batteries.(a) What is the molar mass of sulfuric acid?(b) What is the mass in grams of 1 mole of H2SO4?(c) What is the mass in grams of 2.50 moles of
How many O2 molecules are there in 1.00 g of O2 molecules?
Suppose you wanted 1 billion (1.00 × 109) water molecules and you didn’t have time to sit and count them out. How many grams of water would you need to get 1 billion water molecules?
Consider the balanced chemical equation 2H2O2 → 2 H2O + O2 (a) Given 20.0 g of H2O2 (hydrogen peroxide), how many grams of water will the reaction yield?(b) How many grams of hydrogen peroxide
Consider the balanced chemical equation SCl4 + 2H2O → SO2 + 4 HCl (a) How many grams of H2O will react with 5.000 g of SCl4?(b) How many grams of SO2 can you make from 10.00 g of H2O?(c) Suppose
With 3 cups of flour, 3 cups of sugar, and unlimited amounts of everything else, how many cookies can you make from the recipe in Problem 9.36? Write down your method and cross out units that
Suppose you run the reaction A + 2B → C with B as the limiting reactant and all of the reactants and products are solids. You desire to sell pure product C. What problem are you going to encounter
If you have 25 eggs, 9 blocks of cream cheese, and 4 cups of sugar, how many cakes can you make using the recipe of Problem 9.37? Write down your method and cross out units that cancel.Data from
Consider the following balanced chemical equation:2 H2 + O2 → 2 H2O (a) How many grams of water are formed from 5.00 g of H2 and an excess amount of O2?(b) How many grams of O2 do you need to
Consider the following unbalanced chemical equation: P + O2 → P2O5(a) How many grams of phosphorus (P) are required to react completely with 20.0 g of O2?(b) What is the theoretical yield in grams
Consider the following unbalanced chemical equation:H2 + N2 → NH3(a) To run this reaction in a balanced fashion, how much nitrogen is required if you start with 10.0 g of H2?(b) How many grams of
A gaseous mixture containing 10.079 g of H2 and 7.00 moles of Br2 react to form HBr.(a) Write a balanced chemical equation for this reaction.(b) Which reactant is limiting?(c) What is the theoretical
Chlorine (Cl2) and fluorine (F2) react to form ClF3. A reaction vessel contains 2.50 moles of Cl2 and 6.15 moles of F2.(a) Write a balanced chemical equation for this reaction.(b) Which reactant is
5.00 g of solid sodium (Na) and 30.0 g of liquid bromine (Br2) react to form solid NaBr.(a) Write a balanced chemical equation for this reaction.(b) Which reactant is limiting?(c) What is the
Chlorine (Cl2) and fluorine (F2) react to form ClF3.A reaction vessel contains 10.00 g Cl2 and 10.00 g F2.(a) Write a balanced chemical equation for this reaction.(b) Which reactant is limiting?(c)
Chlorine (Cl2) and fluorine (F2) react to form ClF3.A reaction vessel contains 10.00 g Cl2 and 10.00 g F2.(a) Write a balanced chemical equation for this reaction.(b) Which reactant is limiting?(c)
Butane (C4H10), used as the fuel in disposable lighters, reacts with oxygen (O2) to produce CO2 and H2O. Suppose 10.00 g butane is combined with 10.00 g O2.(a) Write a balanced chemical equation for
A compound has the empirical formula C2H4O. Its molar mass is about 90 g/mol. What is its molecular formula?
An organic compound of carbon and hydrogen has the empirical formula CH. What is its molecular formula if its molar mass is:(a) 26 g/mol (b) 52 g/mol (c) 78 g/mol
A 1.540-g sample of a liquid is subjected to combustion analysis, yielding 40.00% C and 6.71% H. It may also contain oxygen.(a) What is the empirical formula for this compound?(b) The molar mass of
A 2.230-g sample of a solid is subjected to combustion analysis, yielding 76.59% C and 6.39% H. It may also contain oxygen.(a) What is the empirical formula for this compound?(b) The molar mass of
A 1.000-g sample of a liquid is subjected to combustion analysis, yielding 92.3% C and 7.7% H. It may or may not also contain oxygen.(a) What is the empirical formula for this compound?(b) The molar
A 2.000 g sample of a liquid compound that contains only carbon and hydrogen in its formula is subjected to combustion analysis. From the result, the lab determines that 0.2874 g of the original
A compound used as an insecticide that contains only C, H, and Cl is subjected to combustion analysis, yielding 55.55% C and 3.15% H.(a) What is the empirical formula of this compound?(b) What is the
A compound used as an insecticide that contains only C, H, and Cl is subjected to combustion analysis, yielding 24.78% C and 2.08% H.(a) What is the empirical formula for this compound?(b) What is
Determine the empirical formula of the compound with the following mass percents of the elements present: 66.63% C; 11.18% H; 22.19% O.
Determine the empirical formula of the compound with the following mass percents of the elements present: 58.5% C; 4.91% H; 19.5% O; 17.1% N.
Determine the empirical formula of the compound that is 26.4% by mass Na, 36.8% by mass S, and also contains oxygen.
Determine the empirical formula of the compound that is 43.2% by mass K, 39.1% by mass Cl, and also contains oxygen.
Ethanol, the alcohol in beer and wine, has the molecular formula C2H6O. Calculate the mass percent of each element in ethanol.
Ethylene glycol, used for antifreeze, has the molecular formula C2H6O2. Calculate the mass percent of each element in ethylene glycol.
The compound P4O10 has an empirical formula of P2O5. By what factor will the percent by mass composition differ for each element between these two formulas? Explain your answer.
The thyroid hormone thyroxine has the molecular formula C15H11NO4I4. Calculate the mass percent of each element in thyroxine.
(a) What is the molar mass of ribose (C5H10O5)?(b) What is the mass of 3.87 moles of ribose?(c) How many ribose molecules are there in 3.87 moles?(d) How many oxygen atoms are there in 3.87 moles of
Which has more mass:(a) One atom of sulfur or one molecule of oxygen gas (O2)?(b) 0.125 mole of sulfur molecules (S8) or 0.670 mole of ozone (O3)?
Can the actual yield ever be greater than the theoretical yield for a chemical reaction?

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