Q: A compound has an epirical formula of CH2O. If the molar mass of the compound is 60g/mol, what is…
A: emperical mass=12+2+16=30 n=60/2=2
Q: What is the mass, in grams, of 9.84x1024 molecules of methanol (CH3OH)?
A: Given:Number of atoms = 9.84x1024 atoms.Molar mass of CH3OH = 32 g/mol.
Q: What mass of c37h49n2o12 would contain 4.35g of oxygen? What is the mass of exactly 1500 molecules…
A: Answer:- This question is answered by using the simple concept of calculation of molar mass using…
Q: If an experiment produced 3.57 x 10^4 grams of methanol, but calculations performed referencing a…
A: Answer:- This question is answered by using the simple concept of calculation of percent yield using…
Q: A three-step process for producing molten iron metal from Fe2O3 is: 3Fe2O3 + CO → 2Fe3O4 + CO2…
A: Given,The three-step process for producing molten iron metal from Fe2O3 is:3 Fe2O3 + CO → 2 Fe3O4 +…
Q: If you could drop 12 atoms of copper into a beaker containing nitric acid, how many molecules of NO…
A: Copper, Cu(s) when added to dilute nitric acid, HNO3(aq) produces nitric oxide gas, NO(g).
Q: For the reaction C + 2H2 → CH4, how many moles of hydrogen are needed to make 182 grams of methane,…
A: Here a chemical reaction is given that is C + 2H2 → CH4. Now, we have to calculate how many moles…
Q: If a student reacts 41.2 moles of Cl2 with an excess of CH4 how many moles of CCl4 will be produced
A: Synthesis reaction of CCl4 ; CH4 + 4Cl2 ---> CCl4 + 4HCl Moles of Cl2 given = 41.2 moles
Q: Balanced chemical equations relate reactants and products by what quantity?
A: Concept Introduction: Balanced chemical equation gives the details about the identities (moles) of…
Q: Fermentation is a complex chemical process of wine making in which glucose is converted into ethanol…
A:
Q: Suppose that 6.71 × 10³ g of titanium(IV) chloride is reacted with 2.45 × 10° g of oxygen. Calculate…
A:
Q: 3. If 0.4352 grams sample of Copper oxide is heated and decomposes into 0.3477 g of copper and an…
A: Percentage of one element in a sample can be determined by the following way : Mass of that…
Q: In one process, 124 g of Al reacts with 601 g of Fe2O3, what is the mass of Al2O3 formed? 2Al +…
A: The given reaction is 2Al + Fe2O3=Al2O3 + 2Fe Moles of Al =124/27 =4.6moles Moles of Fe2O3 =601/160…
Q: Complete combustion of 7.607.60 g of a hydrocarbon produced 23.323.3 g of CO2 and 11.111.1 g of H2O.…
A:
Q: In a combustion,27.90 g CH4 combine with 110.5 g O2 to make 76.50g CO2 and 62.65g H2O. Does this…
A: As mass in reactant and product side is not equal so it does not follow law of conservation of mass.
Q: How many moles of tetracycline (C₂₂H₂₄N₂O₈) are in 92.1 grams?
A: Before going to find out moles of tetracycline, We first find out molecular weight of C22H24N2O8 ,…
Q: Combustion analysis of 0.800 grams of an unknown hydrocarbon yields 2.613 g CO2 and 0.778 g H2O.…
A: Combustion refers to the process where a substance burns in the presence of oxygen, giving off heat…
Q: What is the mass of carbon present in 0.283 grams of propane (C3H8)?
A: Given data : Mass of propane = 0.283 gram To find : Mass of carbon present in 0.283 grams of…
Q: Combusting an unknown hydrocarbon produces 5 mol CO2 and 6 mol H2O. What is the empirical formula of…
A:
Q: Complete combustion of 5.80 g of hydrocarbon produced 17.8 g of CO2 and 8.49 g of H2O. What is the…
A: Empirical formula is the smallest atom ratio by which a compound can be represented.
Q: A 345.21 g sample of a compound was found to contain 200.50 g of carbon and 144.71 g of hydrogen.…
A: We have 345.21 g of given compound, we have 200.50 g of C, 144.71 g of H. We have to calculate the…
Q: What mass of acetylene, C2H2, will be produced from the reaction of 38.3 g calcium carbide, CaC2,…
A: Given :- mass of CaC2 = 38.3 g To calculate :- mass of C2H2 number of moles = mass/molar mass…
Q: Q21) A 0.1647- gram sample of a pure hydrocarbon was burned in a C- H combustion train to produce…
A: Since all the carbon in carbon dioxide and all the hydrogen in water will come from the hydrocarbon…
Q: experiment was done to determine the composition of a mixture of sodium chloride and sodium…
A:
Q: Complete combustion of 2.90 g of a hydrocarbon produced 8.94 g of CO, and 4.12 g of H,O. What is the…
A: Given Mass of hydrocarbon = 2.90 gram Mass of CO2 = 8.94 gram Mass of H2O = 4.12 gram Empirical…
Q: the combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g h2o and 3.5927 g co2. what is the…
A: Given, Combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H2O and 3.5927 g CO2. Then,…
Q: A 58.5 g sample of an unknown compound that contains only carbon, hydrogen and oxygen was analyzed…
A: Given: The mass of the unknown compound is 58.5 g The mass of CO2 (carbon dioxide) is 105.6 g The…
Q: C6H12O6 + 6O2 → 6CO2 + 6H2O How many grams of glucose are burned to produce the 6 moles of…
A:
Q: The combustion of 1.66 g ultrafine aluminum in air results in 2.97g of a product, which is a mixture…
A: Given: Mass of Aluminium = 1.66 gMass of the product = 2.97 g% of aluminium oxide = 80% of aluminium…
Q: A molecule has an empirical formula of Ch2. 1.34 moles of the compound give 530.76 g of CO2 upon…
A: Given : We have to calculate the molecular formula.
Q: Combustion of 10.68 mg of the compound yields 15.92 mg CO2 in 4.89 mg each to the molar mass of the…
A:
Q: 39.5 g of cobalt will combine with 107 g of bromine to form a binary compound. How much of the same…
A:
Q: What is the mass, in grams, of 9.35×1024 molecules9.35×1024 molecules of methanol (CH3OH)?
A: Given information: molecules of methanol (CH3OH) = 9.35×1024
Q: The compound dioxane, which is used as a solvent in variousindustrial processes, is composed of C,…
A: Molar mass of the given compound is 88.1 g/mol.
Q: A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces 33.5 mg CO2…
A: Given: compound contains only C, H, and N mass of compound = 35 mg mass of CO2 produced = 33.5 mg…
Q: While completing your research on the speciation of clover in Sacramento County, you isolate ah acid…
A: Given compound has only C,H and O elements in it. Mass taken of compound = 0.513 g Mass of carbon…
Q: A three-step process for producing molten iron metal from Fe203 is: 1. 3FE203 + CO –→ 2FE304 + CO2…
A:
Q: The following diagram represents the collection of CO2 andH2O molecules formed by complete…
A: Combustion of hydrocarbon means heating a hydrocarbon in the presence of oxygen to give CO2 and H2O…
Q: The molecular formula for glucos is C6H12O6 and BENZENE HAVE C6H6. What are their respective…
A: The empirical formula of a compound is called the simplest formula. It represents the relative or…
Q: A sample of 10.5g nitrogen reacts with 20.2 grams of hydrogen to produce ammonia. 3H2(g) + N2(g)…
A: Limiting reagent determination find ratio of mol and stoichiometric coefficient, which will have…
Q: The mass of C3H8O3 that can be made from 2.4 × 1023 H atoms is
A:
Q: Combustion of hydrocarbons such as nonane (C,H20) produces carbon dioxide, a "greenhouse gas."…
A: When a hydrocarbon reacts with oxygen then, it will form carbon dioxide and water and liberate huge…
Q: The production of ethanol for use as a fuel can be accomplished through fermentation of glucose, a…
A: The balanced reaction given is C6H12O6(s) → 2CH3CH2OH(l) + 2CO2(g) Hence we can say that 1 mole…
Q: Table salt, NaCl(s), and sugar, C,,H„0(s), are accidentally mixed. A 5.50 g sample is burned, and…
A: Balanced Combustion reaction of sugar: C12H22O11 + 12O2 .....> 12CO2 + 11H2O Mass of sample =…
Q: compound
A: Molar mass of Fe2O3 = 2 • ( molar atomic mass of Fe ) + 3 • ( molar atomic mass of Oxygen atom )…
Q: An empty propane tank weighs 7.22 kg. When it is filled, the tank weighs 25.20 kg How many propane…
A:
Q: Question attached
A: The limiting reagent (or limiting reactant or limiting agent) in a chemical reaction is a reactant…
Q: Question attached
A: Given: Mass of ethanol = 18.5g To find: The number of molecules present in 18.5 g of CH3CH2OH
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- A sample of a hydrocarbon (a compound consisting of only carbon and hydrogen) contains 2.59 1023 atoms of hydrogen and is 17.3% hydrogen by mass. If the molar mass of the hydrocarbon is between 55 and 65 g/mol, what amount (moles) of compound is present, and what is the mass of the sample?Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
- Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l)+O2(g)CO2(g)+H2O(l) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): :math>C5H12(l)+O2(g)CO2(g)+H2O(l) a 20.4-gram sample of pentane is burned in excess oxygen, what mass of water can be produced, assuming 100% yield?A sample of an oxide of vanadium weighing 4.589 g was heated with hydrogen gas to form water and another oxide of vanadium weighing 3.782 g. The second oxide was treated further with hydrogen until only 2.573 g of vanadium metal remained. (a) What are the simplest formulas of the two oxides? (b) What is the total mass of water formed in the successive reactions?
- Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid fuel rocket motors. The reaction is :math>Fe2O3(s)+2Al(s)2Fe(l)+Al2O3(s) l type='a'> What mass of iron(III) oxide must be used to produce 25.69 g of iron? What mass of aluminum must be used to produce 25.69 g of iron? What is the maximum mass of aluminum oxide that could be produced along with 25.69 g of iron?Using Chemical Equation Coefficients as Conversion Factors (Mass to Mass) One of the reactions occurring in automobile engines is the combustion of octane (C8H18): 2C8H18+25O216CO2+18H2O Assume that gasoline is pure octane and that you burn approximately 6.44104 grams of octane per week (about 20 gal). How many grams of CO2 are produced?Consider the following reaction: 4NH3(g)4NO(g)+6H2O(g) If a container were to have 10 molecules of O2 and 10 molecules of NH3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?
- A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.3.55 An average person inhales roughly 2.5 g of O2 in a minute. How many molecules of oxygen are inhaled in (a) 1 minute, (b) 1 hour, (c) 1 day by an average person?Nitrogen fixation in the root nodules of peas and other legumes occurs with a reaction involving a molybdenum-containing enzyme named nitrogenase. This enzyme contains two Mo atoms per molecule and is 0.0872% Mo by mass. Calculate the molar mass of the enzyme.