Propane gas and oxygen gas will chemically react via combustion. Write a blanced equation for this change and then use stoichiomety problem solving to determine the number of carbon dioxide molecules that can theoretically form.
The balanced equation for the combustion of propane gas (C₃H₈) with oxygen gas (O₂) is:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
To determine the number of carbon dioxide (CO₂) molecules that can theoretically form in this reaction, we need to use stoichiometry calculations.
From the balanced equation, we can see that one molecule of propane (C₃H₈) reacts with five molecules of oxygen (O₂) to produce three molecules of carbon dioxide (CO₂). This means that the stoichiometric ratio between propane and carbon dioxide is 1:3.
To calculate the number of carbon dioxide molecules that can theoretically form, we need to know the amount of propane present. Let's assume we have x molecules of propane.
Using the stoichiometry ratios, we can set up a proportion:
1 molecule C₃H₈ / x molecules C₃H₈ = 3 molecules CO₂ / y molecules CO₂
Cross-multiplying, we get:
y = (3 * x) / 1
y = 3x
Therefore, the number of carbon dioxide molecules that can theoretically form is three times the number of propane molecules present.
To write a balanced equation for the reaction between propane gas (C3H8) and oxygen gas (O2), we first need to understand their chemical formulas and the products of their combustion.
The chemical formula for propane gas is C3H8, which means it contains three carbon (C) atoms and eight hydrogen (H) atoms. The chemical formula for oxygen gas is O2, indicating it consists of two oxygen (O) atoms bonded together.
When propane gas reacts with oxygen gas, the products are carbon dioxide (CO2) and water (H2O). The balanced equation for this combustion reaction can be written as follows:
C3H8 + 5O2 -> 3CO2 + 4H2O
To determine the number of carbon dioxide molecules that can theoretically form in this reaction, we need to use stoichiometry. Stoichiometry is a branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction.
From the balanced equation, we can see that for every 3 molecules of carbon dioxide (CO2) formed, we need 1 molecule of propane (C3H8). Therefore, the stoichiometric ratio of CO2 to C3H8 is 3:1.
To calculate the number of carbon dioxide molecules that can form, we need to know the number of propane molecules. Let's assume we have 10 molecules of propane.
First, we convert the number of propane molecules to moles using the molar mass of propane, which is 44.1 grams/mole. As 1 mole of any substance contains 6.022 x 10^23 molecules (Avogadro's number), we can use this conversion factor to determine the number of moles of propane:
10 molecules C3H8 x (1 mole C3H8 / 6.022 x 10^23 molecules C3H8) = 1.66 x 10^-22 moles C3H8
Now we can use the stoichiometric ratio to calculate the number of moles of carbon dioxide:
1.66 x 10^-22 moles C3H8 x (3 moles CO2 / 1 mole C3H8) = 4.99 x 10^-22 moles CO2
Finally, we convert the moles of carbon dioxide to molecules using Avogadro's number:
4.99 x 10^-22 moles CO2 x (6.022 x 10^23 molecules CO2 / 1 mole CO2) = 3.01 molecules of CO2
Therefore, theoretically, 3.01 carbon dioxide molecules can form from the combustion of 10 molecules of propane.