200.0 g of a pure hydrocarbon was combusted in oxygen.  The reaction was a complete combustion.  This resulted in the production of 606.9 g of carbon dioxide and 310.3 g of water.  A mass spectrum of the hydrocarbon indicated that the molar mass is 58 g/mol.  Based on this information, determine the molecular formula of the hydrocarbon.

The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of phosphorus trichloride that can be formed from 226.0 grams of chlorine gas based on the balanced chemical equation?

A hydrated sample of sodium hydrogen phosphate (Na2HPO4) was found to contain 47.05% water by mass. Determine the formula of the hydrate. Molar mass of anhydrous sodium hydrogen phosphate (Na2HPO4) = 141.96 g/mol Molar mass of water H2O = 18.015g/mol

The chemical equation for the combustion of butane is 2 C4H10(g) + 13 O2(g) = 8 CO2(g) + 10 H2O(g) Predict what mass of carbon dioxide is produced from 10.0g of butane and 30.0g of oxygen.

Given the following balanced chemical equation:                       Zn + 2 HCl → ZnCl2 + H2 Calculate the mass in grams of H2 will be produced, if 25.0 grams of Zn are reacted with 17.5 g of HCl.

A classic SUV features a 194 L gas tank. Assuming a molecular formula of C8H18 for gasoline and complete combustion of the gasoline with O2 to form CO2 and H2O, calculate the amount of O2 in kilograms consumed per tank of gasoline. Assume a density of 780 g/L for the gasoline.   Atomic Mass: C: 12.011 g/mol H: 1.008 g/mol O: 15.999 g/mol   Round your answer to 2 decimal places.

A mixture of C2H2 and CH4 has a total mass of 164 g. When this mixture reacts completely with excess oxygen, the CO2 and H2O products have a combined mass of 746.6 g. What mass of CH4 was present in the initial mixture?

Complete combustion of 2.50 g of a hydrocarbon produced 8.04 g of CO2 and 2.74 g of H2O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary.

1.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 180. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass 1.47 g carbon dioxide 0.60 g water Use this information to find the molecular formula of X.

Complete combustion of 7.70 g of a hydrocarbon produced 23.7 g of CO2 and 10.9 g of H2O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary.