A compound is made up of 168.2 g Cd, 35.96 g C, 4.53 g H, and 47.91 g O. What is the empirical formula of this compound? Provide your answer below:
A compound has a mass percentage of 53.46% C, 6.98% H, and 39.56% O. What is the empirical formula for this compound? Provide your answer below:
Citric acid contains 37.51% C, 4.20% H, and 58.29% O by mass. What is the empirical formula of this compound? Provide your answer below:
A compound is made up of 28 g N, 24 g C, 48 g O, and 8 g H. What is the empirical formula? Provide your answer below:
A compound that weighs 56.2 g contains 23.6 g Sb (antimony) and 32.6 g F (fluorine). What is the percent composition of antimony? Your answer should have three significant figures. Provide your answer below:
A 36.0 g sample contains 14.6 g Cl and 21.4 g B. What is the percent composition of chlorine in this sample by mass? Your answer should have three significant figures. Provide your answer below: %
A 15.8 g sample contains 3.6 g F, 4.9 g H, and 7.3 g C. What is the percent composition of carbon in this sample? Your answer should have two significant figures. Provide your answer below: %
A compound that weighs 40.8 g contains 23.6 g Sb and 17.2 g F. What is the percent composition of fluorine? Your answer should have three significant figures. Provide your answer below: %
A sample of a compound is made up of 57.53 g C, 3.45 g H, and 39.01 g F. Determine the empirical formula of this compound. Provide your answer below:
A 150 g sample of a compound is comprised of 44% C, 9% H and the remainder is O by mass. What is the compound's empirical formula? Hint: The percentage of all three elements must add up to 100%. Provide your answer below:
What is the empirical formula of a compound with a percent composition of 4.7% N, 7.1% H, 72.2% C, and 16.0% O ? Provide your answer below:
A compound has a molecular weight of 477.18 g/mol and an empirical formula of C10H7O2. What is the molecular formula? Select the correct answer below: C30H21O6 C4H13O3 C14H12O3 none of the above
Jacob finds that a compound has a molar mass of 128 g/mol and an empirical formula of SO2. What is the molecular formula of this compound? Select the correct answer below: S2O3 S2O4 S3O4 SO2
The formula of nitric acid is HNO3. Determine the percent composition of hydrogen in this compound. Round your answer to three decimal places. Provide your answer below:
Ammonium nitrite (NH4NO2) has a percent composition of for oxygen. Select the correct answer below: 44.91% 53.20% 48.52% 49.96%
Antimony pentafluoride has a formula of SbF5. What is the percent composition of F in this molecule? Round your answer to three decimal places. Provide your answer below:
The formula of a compound is H2 CO3. Determine the percent composition of carbon in this compound. Your answer should have two significant figures. Provide your answer below: %
The empirical formula of a compound is CH2O and its molecular weight is 90.09 g/mol. Determine the molecular formula. Provide your answer below:
The molecular weight of a compound is 140 g/mol. If the empirical formula is C4H6O, what is the molecular formula? Provide your answer below:
What is the empirical formula of a compound that contains 10.0 g aluminum and 8.88 g oxygen? Select the correct answer below: AlO3 Al2O3 AlO1.5 Al2O
A 2.00 g sample of unknown hydrocarbon is found to contain 1.50 g carbon and 0.50 g hydrogen. What is the compound's percent composition by mass? Select the correct answer below: 75% carbon, 25% hydrogen 25% carbon, 75% hydrogen 50% carbon, 50% hydrogen 67% carbon, 33% hydrogen
What is the empirical formula of a compound that is 20.2% aluminum and 79.8% chlorine by mass? Select the correct answer below: AlCl AlCl2 AlCl3 AlCl4
What is the percent by mass of oxygen in potassium permanganate ( KMnO4 ) Select the correct answer below: 14.52%O 58.20%O 40.50% O 10.14% O
What is the molecular formula of ethane, a hydrocarbon that is 80.0% carbon and 20.0% hydrogen by mass? The molar mass of ethane is 30 g/mol. Provide your answer below:
Identify the balanced chemical equation. Select the correct answer below: 2 Fe2O3 + 3C → 4Fe + 3CO2 H2O2 → H2O + O2 SO2 + O2 + H2O → 4H2 SO4 2Mg + HCl → MgCl2 + H2
4Fe + 3O2 → 2Fe2O3 Using the chemical equation provided, identify the coefficient of the product. Select the correct answer below: 7 4 3 2
Using the chemical equation provided, identify which of the following are the reactants. Select all that apply. 4Fe + 3O2⟶2Fe2O3 Select all that apply: Fe O2 Fe2O3 All of the above
Fill in the blank with the coefficient for CO2 in the balanced version of the following chemical equation: C4H10O + O2 → CO2 + H2O Your answer should be a whole number. Provide your answer below:
Using the chemical equation provided, identify which of the following are the coefficients of the reactants. 4Fe + 3O2 ⟶ 2Fe2O3 Select all that apply: 7 4 3 2
In a chemical equation, the number of atoms of a particular element that are present in a substance is indicated by a: Select the correct answer below: coefficient forward arrow plus sign subscript
Consider the following chemical equation. C2H6 + O2 → CO2 + H2O What will be the coefficient for CO2 in the balanced equation? Type your answer as a whole number. The balanced equation will have all coefficients as whole numbers. Provide your answer below:
Fill in the blanks to give the balanced version of the following chemical equation: NH4NO2 → N2 + H2O Your answers should be whole numbers. Provide your answer below: NH4NO2 → N2 + H2O
What is the net ionic equation for the following balanced reaction: K2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2KCl(aq) Please include the charges for the ions. Provide your answer below: (aq) + (aq) → (s)
Solid nickel reacts with aqueous lead (II) nitrate to form solid lead. What is the net ionic equation for this reaction? Hint: In this reaction, nickel exhibits its most common oxidation state of +2. Be sure to include the charge for each ion in the net ionic equation. Provide your answer below: (s) + (aq) → (aq) + (s)
What is the net ionic equation for the following reaction that takes place in water? Mg + H2SO4 ⟶ MgSO4 + H2 Include charges on ions. Provide your answer below: Mg(s) + 2(aq) → (aq) + H2(g)
Hydrochloric acid dissolves solid aluminum hydroxide. What is the complete ionic equation of this reaction? Select the correct answer below: 3 HCl + Al(OH)3(s) → 3 H2O(l) + AlCl3(aq) 3H+ + 3Cl− + Al(OH)3(s) → 3H2O(l) + Al3+ + 3Cl− 3H+ + Al(OH)3(s) → 3H2O(l) + Al3+ none of the above
Aqueous potassium carbonate reacts with aqueous silver nitrate to precipitate silver carbonate. What is the net ionic equation of this reaction? Include charges on ions. Provide your answer below: 2(aq) + CO32−(aq) → (s)
How many grams of S8 is required to produce 83.10 gSF6 ? S8 + 24F2 ⟶ 8SF6 Your answer should have four significant figures. Provide your answer below: g
What mass of Fe is required to produce 32.00 g Fe2O3 ? 4Fe + 3O2 ⟶ 2Fe2O3 Your answer should have four significant figures. Provide your answer below:
How many molecules of NO2 will be generated when 3.80 moles of oxygen react according to the following equation: 2NO + O2 → 2NO2 Use 6.022×1023 mol−1 for Avogadro's number. Your answer should have three significant figures. Provide your answer below: molecules
How many moles of CuSO4 are required to react with 2 moles Fe ? Fe + CuSO4 ⟶ Cu + FeSO4 Select the correct answer below: 0.5 1 2 4
According to the given reaction, how many molecules of S8 are required to react with 4.87 moles F2 ? S8 + 24F2 ⟶ 8SF6 Use 6.022×1023 mol−1 for Avogadro's number. Your answer should have three significant figures. When using scientific notation to report your answer use the multiplication symbol, ×, not the letter x Provide your answer below: molecules
From the following balanced equation, 2 Al(s) + 3 Cl2(g)⟶2 AlCl3(s) how many moles of Cl2 are required to form 3.55 mol AlCl3 ? Your answer should have three significant figures. Provide your answer below: mol
According to the given equation, how many moles of iron are required to react with 0.85 moles oxygen? 4 Fe + 3 O2 ⟶ 2 Fe2O3 Your answer should have two significant figures. Provide your answer below: mol
How many moles of HCl are required to react with 2.5 mol of Zn ? Zn + 2 HCl ⟶ ZnCl2 + H2 Report your answer with two significant figures. Provide your answer below: mol
According to the below equation, how many moles of P2H4 will be required to generate 1.76×1023 molecules of P4 ? 6P2H4 → 8PH3 + P4 Use 6.022×1023 mol−1 for Avogadro's number. Your answer should have three significant figures. Provide your answer below: mol
According to the given equation, how many molecules of H2 are required to produce 3.2 moles HCl ? H2 + Cl2 ⟶ 2 HCl Use 6.022×1023 mol−1 for Avogadro's number. Your answer should have two significant figures. Provide your answer below: molecules
If 3.82 g aluminum react, how many grams of aluminum oxide can we expect according to the following equation: 4Al + 3O2 → 2Al2O3 Your answer should have three significant figures. Provide your answer below:
What mass of C2H6 is necessary to produce 280.0 g CO2 in the following reaction? 2 C2H6 + 7 O2 ⟶ 4 CO2 + 6 H2O Your answer should have four significant figures. Provide your answer below: g
What is the percent yield of NH3 if a reaction starts with 77.0 g CaCN2 and produces 27.1 g NH3 ? CaCN2 + 3 H2O ⟶ CaCO3 + 2 NH3 Select the correct answer below: 76.4% 82.8% 89.47% 93.20%
What is the percent yield of iron(II) chloride (FeCl2) if we start with 34 gFeBr2 and produce 4.0 gFeCl2 ? FeBr2 + 2 KCl ⟶ FeCl2 + 2 KBr Select the correct answer below: 11% 18% 20% 37%
44 g I2O5 combine with 100 gBrF3. Which is the limiting reactant? 6I2O5 + 20BrF3 → 12IF5 + 15O2 + 10Br2 Select the correct answer below: BrF3 I2O5 IF5 O2
1.0 g P4O10 combines with 2.0 g PCl5. Which is the limiting reactant? P4O10 + 6PCl5 → 10POCl3 Use elemental symbols for your answer. Provide your answer below:
The limiting reactant will always be: Select the correct answer below: the reactant present in lesser quantity the reactant present in greater quantity the reactant that runs out first the reactant that remains after a reaction
10 g sucrose and 10 g oxygen are reacting. Which is the limiting reactant? C12H22O11 + 12O2 → 12CO2 + 11H2O Select the correct answer below: sucrose carbon dioxide oxygen water
If the theoretical yield of a reaction is 100 grams, which value for actual yield is physically impossible? Select the correct answer below: 0 grams 50 grams 99.9 grams 110 grams
If the actual yield for a reaction is 15.0 g, and the percent yield for the reaction is 60.0%, what is the theoretical yield for the reaction? Your answer should have three significant figures. Provide your answer below:
In the chemical equation A + B ⟶ C + D, which are products? Provide your answer below: and
When aqueous solutions of NH4 OH(aq) and CuCl2(aq) are mixed, the products are NH4 Cl(aq) and Cu(OH)2(s). What is the net ionic equation for this reaction? Select the correct answer below: 2NH4OH(aq) + CuCl2(aq) ⟶ Cu(OH)2(s) + 2NH4 Cl(aq) 2NH4+(aq) + 2OH−(aq) + Cu2+(aq) + 2Cl−(aq) ⟶ Cu(OH)2(s) + 2 NH4+(aq) + 2 Cl−(aq) Cu2+(aq) + 2OH−(aq) ⟶ Cu(OH)2(s) NH4+(aq) + Cl−(aq) ⟶ NH4 Cl(s)
Fill in the blanks with the coefficients for the balanced version of the following equation: C8H18 + O2 ⟶ CO2 + H2O Your answers should be whole numbers. Provide your answer below: C8H18 + O2 → CO2 + H2O
From the following balanced equation, 4 NH3(g) + 5 O2(g) ⟶ 4 NO(g) + 6 H2O(g) how many moles of H2O can be formed from 3.78 mol O2 ? Select the correct answer below: 3.15 mol 4.54 mol 4.73 mol 3.02 mol
From the following balanced equation, 2 Na(s) + Cl2(g) ⟶ 2 NaCl(s) how many moles of NaCl can be formed from 3 mol Cl2 ? Your answer should have one significant figure. Provide your answer below: mol
From the following balanced equation, CH4(g) + 2 O2(g) ⟶ CO2(g) + 2 H2O(g) how many grams of H2O can be formed from 1.25 g CH4 ? Your answer should have three significant figures. Provide your answer below: g
From the following balanced equation, CH4(g) + 2 O2(g) ⟶ CO2(g) + 2 H2O(g) how many grams of H2O can be formed when 1.25 g CH4 are combined with 6.66 g O2 ? Your answer should have three significant figures. (Round your answer to second decimal place). Provide your answer below: grams