# Problem: An organic compound was found to contain only C, H, and Cl. When a 1.60 -g sample of the compound was completely combusted in air, 3.75 g of CO2 was formed. In a separate experiment the chlorine in a 1.30 -g sample of the compound was converted to 1.65 g of AgCl.Determine the empirical formula of the compound.

###### FREE Expert Solution

We’re being asked to determine the empirical formula of a compound composed of C, H, and Cl given the combustion analysis, a 1.60-g sample is combusted to produce 3.75 g of COand in a separate experiment, the chlorine in a 1.30-g sample was converted into 1.65-g AgCl

Recall that in combustion analysisa compound reacts with excess O2 to form products

For a compound composed of C, H the reaction looks like this:

CxHyClz + O2 (excess) x CO2 + y H2O+ z HCl

This means we need to do the following steps:

Step 1: Calculate the mass of C in the compound from combustion.

Step 2: Calculate the mass of Cl in the compound from the reaction.

Step 3: Calculate the mass of H by subtracting the mass of C and Cl from the total mass.

Step 4: Determine the lowest whole number ratio of C, H, and Cl to get the empirical formula.

81% (352 ratings) ###### Problem Details

An organic compound was found to contain only C, H, and Cl. When a 1.60 -g sample of the compound was completely combusted in air, 3.75 g of CO2 was formed. In a separate experiment the chlorine in a 1.30 -g sample of the compound was converted to 1.65 g of AgCl.

Determine the empirical formula of the compound.