Consider the following balanced equation for the following reaction:
15O2(g) + 2C6H5COOH(aq) → 14CO2(g) + 6H2O(l)
Determine the amount of CO2(g) formed in the reaction if the percent yield of CO2(g) is 83.0% and the theoretical yield of CO2(g) is 1.30 moles.

The actual yield of the carbon dioxide is 47.48 grams

Explanation:

For the given balanced equation:

To calculate the mass for given number of moles, we use the equation:

Theoretical moles of carbon dioxide = 1.30 moles

Molar mass of carbon dioxide = 44 g/mol

Putting values in above equation, we get:

To calculate the theoretical yield of carbon dioxide, we use the equation:

Theoretical yield of carbon dioxide = 57.2 g

Percentage yield of carbon dioxide = 83.0 %

Putting values in above equation, we get:

Hence, the actual yield of the carbon dioxide is 47.48 grams

it is to be noted that an alpha particle is an helium nucleus. so it contains 2 protons 2 neutrons and has a mass number of 4. when alpha decay particles are ejected from the nucleus it gets transformed into an atom which has atomic number less than 2 and a mass number less than 4.

an equation that could represent alpha decay is radium 226 decay of alpha particle forms radon 222.

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