Combustion analysis of a 2.50 g sample of a compound containing only carbon, hydrogen and nitrogen produces 7.09 g of CO2 and 1.69 g of H₂O. Calculate the empirical formula of the compound (CxHyNz). A You do not need to put 1's in the formula. You do not need to subscript numbers in the formula. For example, H₂O would be written as H2O.

Q: Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium…

A: First we will write balanced equation, then using it calculate the amount of reactants left after…

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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.…

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Q: The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane…

A: Combustion reaction of octane 2C8H18 + 25O2 → 16CO2 + 18H2O From this Balanced chemical equation we…

Q: When 3.433 grams of a hydrocarbon, C,Hy, were burnec in a combustion analysis apparatus, 10.52 grams…

A: Mass of Hydrocarbon = 3.433 grams Molar mass of Hydrocarbon = 86.18 grams Number of moles of…

Q: Combustion analysis of a hydrocarbon produced 33.01 g CO2 and 4.83 g H2O. Calculate the empirical…

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Q: Para-cresol, a substance used as a disinfectant and in the manufacture of several herbicides, is a…

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Q: A compound containing the elements C , H , N , and O is analyzed. When a 1.2359 g sample is burned…

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Q: Gaseous butane  CH3CH22CH3  will react with gaseous oxygen  O2  to produce gaseous carbon dioxide…

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Q: common organic solvent, gives 7.62 mgmg of CO2CO2 and 1.78 mgmg of H2OH2O. If the compound contains…

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Q: A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields…

A: The number of moles of the compound can be calculated by dividing the given mass of the compound by…

Q: A beaker contains 100.0 mL of water. To it is added 10.0 mL of dilute nitric acid (HNO3). Calculate…

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Q: Vitamin C, an antioxidant present in citrus fruits, contains only C, H, and O. Combustion of 10.0 g…

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Q: Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be…

A: Calculate the number of moles of HBr and NaOH Number of moles = Given massMolar massNumber of moles…

Q: A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces 53.0 mg CO2 and…

A: Given: Compound contains only C, H and N. Mass of compound combusted = 35.0 mg = 0.035 g.…

Q: During a chemical reaction tin and iodine combine to form an orange solid. If the resulting tin…

A: Given,

Q: Aqueous sulfuric acid (H₂SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous…

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Q: The balanced equation below shows the reaction which occurs between silver nitrate and sodium…

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Q: How

A: moles of water = ( molecules of water ) / ( Avogadro number )  Where :  Molecules of water is 2.0 •…

Q: 1)Copper metal reacts with molecular nitrogen to form copper(II) nitride.  a)Write the balanced…

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Q: 3. What is the mass (in kg) of 6.89 x 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol.

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Q: Complete combustion of 7.70 g of a hydrocarbon produced 23.7 g of CO2 and 10.9 g of H2O. What is the…

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Q: Vitamin C, an antioxidant present in citrus fruits, contains only C, H, and O. Combustion of 10.0 g…

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Q: 21.2 g sample of a compound that contained carbon, hydrogen, and oxygen was burned in excess oxygen.…

A: Mass of CO2 = 26.40 g Mass of H2O= 10.80 g Moles of CO2 = Mass / Molecular weight Moles of CO2 =…

Q: 0.333 g of a hydrocarbon (CxHy) was analyzed by combustion analysis and 1.009 g of CO2 (MM = 44.01…

A: Answer:- This question is answered by using the simple concept of calculation of moles using the…

Q: A 6.40 g sample of a compound is burned to produce 8.37 g CO, 2.75 g HO, 1.06 g N, and 1.23 g SO.…

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Q: The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane…

A: The balanced form of equation will be -2C8H18g+25O2g→18H2Og+16CO2g8.7 kg…

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Q: Convert 1.43 x 10^23 molecules/formula units of X5Z3 into grams of the same compound. (Assume that…

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Q: A chemical compound has 53.657% C, 3.081% H, and rest of oxygen. Find the empirical formula of the…

A: GIVEN: %C = 53.657 % % H =3.081 % Vapor density = 850.6 amu To calculate: Molecular formula

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.