Question

determine the empirical formula for a compound that has the following analysis: a 13.07 g sample of an unknown substance is composed of 9.48 g of barium, 1.66 g of carbon, and 1.93 g of nitrogen

Answer 1

Answer: BaC2N2

Explanation: You start with your grams and divide them by their mass to get moles.

9.48g/137.33=.0690

1.66/12.01=.1382

1.93/14.007=.1379

You then take your moles and divide them by the smallest mole.

.0690/.0690=1

.1382/.0690=2.002

.1379/.0690=1.999

You then multiply them by a whole number to get them to be whole numbers, in this case you can use one.

1*1=1

2.002*1=2.002- round down to 2

1.999*1=1.999- round up to 2.

Answer 2

Empirical Formula for given compound Ba1C2N2.

Step-by-step explanation:

Step 1; convert the mass of each element into their molar values by dividing available mass by molar masses.

Molar masses of required elements are as follows; Ba- 137.327, C- 12, N- 14.

Step 2; Divide all the values by the smallest mole value. For given compound after dividing the masses by molar masses we get 0.0690, 0.1383, 0.1378 for elements Ba, C, N respectively. Divide all three values with the least value which is 0.0690 and note these values.

Step 3; Convert all the numbers available into whole numbers by multiplying with suitable values. i.e. 3 if values are 0.33, 2 if values are 0.5 etc.

Step 4; Assign these values to corresponding elements and you will get the above empirical formula.