Complete combustion of 4.70 g of a hydrocarbon produced 15.1 g of CO2 and 5.15 g of H2O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. empirical formula: ||C,H, Incorrect

Vitamin C, an antioxidant present in citrus fruits, contains only C, H, and O. Combustion of 10.0 g of vitamin C produces 14.99 g of CO₂ and 4.092 g of H₂O. Determine the molar mass of the compound if it is between 150.0 and 220.0 g/mol. Provide an answer to four significant figures.

Ethanol (C,H O) is combusted in air according to the following reaction: C,H,O(1) + O,(g) –→ CO,(g) + H,0(I) How many grams of water would be produced by the complete combustion of 5.07 moles of ethanol in the presence of excess oxygen? + MacBook Pro 888 こニ。 esc & # $ @ 7 2 3 4 R Y Q W E ab F А lock C V option command ontrol cの つ つ エ

how did you get the numbers beside the balanced equations. such as 4 beside H2O and 2 beside N2.

Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with hydrogen gas can be used to produce methanol.A student reacted 51.9 g of H2(g) with excess CO(g) to produce methanol.If his percent yield was 47.7%, calculate the mass (in g) of CH3OH(l) that he collected in the experiment.Hint: Write a balanced chemical reaction equation.Record only your final answer with the correct number of significant digits and the proper units.

Given the reaction: 2C,H, + 70, → 4C0, + 6H,0 What is the total number of moles of CO, produced by the complete combustion of 5.0 moles of C,H,? 2.0mol 1.0mol 5.0mol O 10.mol

the reaction of 15 moles of carbon with 30 moles of oxygen will result in a theoretical yield of ____ moles of CO2 is what?

6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles

For the following reaction: C3H8(g) + 02 ——-> CO2(g) +H20(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams of each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams

The combustion of 135 mg of a hydrocarbon sample produces 440. mg of CO2 and 135 mg H2O. The molar mass of the hydrocarbon sample is 270 g/mol. Determine the molecular formula of the hydrocarbon.