# chemistry

Complete combustion of 4.80 g of a hydrocarbon produced 15.6 g of CO2 and 4.80 g of H2O. What is the empirical formula for the hydrocarbon?

1. 👍
2. 👎
3. 👁
1. Convert to mols C and mols H.
15.6 x (12/44) = ?
4.80 x (2*1/18) = ?
Find the ratio of the two. The easy way to do that is to divide the smaller number by itself, then divide the other number by the same small number. I get 1:1.5 which in small whole numbers is 2:3

1. 👍
2. 👎
2. How do you get a ratio?

1. 👍
2. 👎
3. I slipped up by converting to C first. It can be done that way but it's longer. Let me start over.

Convert 15.6g CO2 to mols. mols = g/molar mass
15.6/44 = 0.354 mols CO2 = 0.354 mols C since there is 1 atom C in 1 molecule CO2.

4.80g H2O to mols.
4.80/18 = 0.2667 mols H2O and mols H will be twice that or 0.2667*2 = 0.533 mols H.

To find the ratio do what I suggested you do. Divide the smaller number by itself (that gives you a 1.00 every time), then divide the other number by the same smaller number.
We have 0.354 mols C
and 0.533 mols H.

0.354/0.354 = 1.00 C
0.533/0.354 = 1.51 H which rounds to 1.5 and that is a ratio of 2C for 3H or the empirical formula is C2H3.
However, let me point out that 4.80g C2H3 will give you 15.6 g CO2 but it will NOT give you 4.80g H2O so I think someone goofed when they constructed the problem. But the above procedure is how you work the problem.

1. 👍
2. 👎

## Similar Questions

1. ### chemistry

which conversion factor do you use first to calculate the number of grams of CO2 produced by the reaction of 50.6 gram of CH4 with O2? The equation for the complete combustion of methane is: CH4+2O2-->CO2+2H2O.

2. ### chemistry

The complete combustion of propane, C3H8(g), is represented by the equation: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ How much heat is evolved in the complete combustion of 20.0 L C3H8(g) at STP?

3. ### chemistry

The complete combustion of ethanol, C2H5OH (FW = 46.0 g/mol), proceeds as follows: C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) ΔH = −555 kJ What is the enthalpy change for combustion of 15.0 g of ethanol

4. ### chemistry

Complete combustion of a 0.40-mol sample of a hydrocarbon, CxHy, gives 2.40 mol of CO2 and 1.60 mol of H2O. The molecular formula of the original hydrocarbon is Group of answer choices C2H8. C6H8. C9H16. C5H5. C4H7.

1. ### ap

Identify the type of reaction C4H10(g) + O2(g) ! CO2(g) + H2O(g) 1. hydrocarbon synthesis 2. single displacement 3. incomplete combustion 4. complete combustion

2. ### Chemistry

0.22g of a hydrocarbon (compound of C & H) on complete combustion with oxygen gave 0.9 g of water and 0.44g carbon dioxide. Show that these are in accordance with law of conservation of mass.

3. ### Chemistry

When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H2O. A)Write the balanced chemical equation for this reaction. B)Which is the limiting reactant?

4. ### Chemistry

Many power plants produce energy by burning carbon-based fuels, which also produces CO2. CO2 is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the

1. ### CHEMISTRY...........

1. If 29.0 L of methane, CH4, undergoes complete combustion at 0.961 atm and 140°C, how many liters of each product would be present at the same temperature and pressure? My answer: (0.961 atm)(29.0 L) (413k) all divided by

2. ### Chemistry Honors

When a Bunsen burner is ignited, it begins a combustion reaction of methane gas in the air. CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (l) How many moles of water will be produced from the complete combustion of 4 moles of methane?

3. ### chemistry

2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g Part B Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product. Part C Calculate the heat produced by combustion per liter of methanol.

4. ### chem

methyl benzene + oxygen is this just a combustion reactions so CO2 and H2O are produced?