A hydrocarbon mixture consists of 85.71% carbon and 14.29% hydrogen by mass. What is the empirical formula of the hydrocarbon? Please express your answer in the form (for example) C2H5 without subscripting formats ("ONES" (1) are not required). Empirical formula: If the molecular weight of the hydrocarbon is approximately 56 g/mol, what is the molecular formula? Please express your answer in the form (for example) C2H5 without subscripting formats ("ONES" (1) are not required). Molecular formula:

The complete combustion of gasoline (C8H18) is best represented by which of the following equations:   2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O(l)   2 C8H18 (l) + 17 O2 (g)  → 16 CO (g) + 9 H2O (l)   C8H18 (l)  → 8 C (s) + 9 H2 (g)   C8H18 (l) + O2(g) → 8 CO2 (g) + 9 H2O (l)   C8H18 (l) + O(g) → 8 CO2 (g) + 9 H2O (l)

The composition of a compound was found to be 66.7% C, 25.9% N and 7.41% H by mass? What is the empirical formula for the compound? If the molar mass was determined to be 108.0 g, what is the molecular formula of this compound? In your answer, be sure to first state the empirical formula followed by the molecular formula.

1) The explosive RDX has the chemical formula C3H6NO6. Balance the following combustion reaction for RDX. C3H6N606(s) _CO(g) + H₂O(g) + N2(g) 2) Based on the above reaction, would you expect RDX to produce a lot of smoke when it is burned?

2HCN(9) + 6H,0 2NH3 (9) 302(9) (g) ----- ----- + + 2CH4 (9) 4. How many Liters of HCN gas can form from the reaction of 1.56 x 10° grams of NH3, 4.5 moles of oxygen gas, and 12.2 Liters of methane gas? What mass of excess reactant remains?

A chemical compound containing hypothetical elements Av, Bw, Cx, Dy, Ez has mass percentages of 20.670% Av, 11.120% Bw, 41.423% Cx, 10.082% Dy, and 16.705% Ez. Determine the molecular formula if the molar mass of the compound is 1422.10 g/mol. Atomic Mass: Av: 18.25 g/mol Bw: 4.32 g/mol Cx: 26.82 g/mol Dy: 8.16 g/mol Ez: 12.48 g/mol Note: Write the answer in this format: Av1Bw2Cx3Dy5Ez5. 1, 2, 3, 4, and 5 are sample answers What is the molecular formula of the compound? Blank 1 Show your solutions in the next item Blank 1 Add your answer

Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid. Write a balanced equation for the reaction. Calculate the theoretical yield of sulfuric acid. Calculate the percent yield of the reaction. (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

Balance the following equations in which ethane, C2H6, burns in oxygen.    C2H6(g) + O2(g) --> C(s) + H2O(g)    C2H6(g) + O2(g) --> CO(g) + H2O(g)    C2H6(g) + O2(g) --> CO2(g) + H2O(g) d.   Explain why the coefficients for oxygen vary, depending on whether C, CO, or CO2 is formed.

The fuel tank of an automobile contains 62.0 kg of gasoline. If the gasoline reacts completely with excess oxygen (from the air) to form CO2 and H2O, what is the total mass of the products? For simplicity, assume that gasoline is comprised of 100% octane.(C8H18).

ту. [References] H2O absorber CO, absorber Sample When 1.699 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus, 5.598 grams of CO2 and 1.528 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 40.06 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula =