If 27 grams of propane react with 88 grams of oxygen to make carbon dioxide and water then how many grams of carbon dioxide can be made?
To determine how many grams of carbon dioxide can be made, we need to calculate the moles of propane and oxygen consumed in the reaction.
1. Obtain the molar mass of propane (C3H8). Carbon has a molar mass of 12.01 g/mol, and hydrogen has a molar mass of 1.01 g/mol. Since propane has three carbon atoms and eight hydrogen atoms, the molar mass of propane is:
(3 * 12.01 g/mol) + (8 * 1.01 g/mol) = 44.11 g/mol
2. Calculate the moles of propane consumed: Divide the mass of propane (27 g) by its molar mass (44.11 g/mol):
27 g / 44.11 g/mol = 0.612 mol
3. Next, determine the moles of oxygen consumed in the reaction. The balanced chemical equation for the reaction is:
C3H8 + 5O2 -> 3CO2 + 4H2O
From the equation, we can deduce that for every mole of propane, 5 moles of oxygen are needed to produce 3 moles of carbon dioxide. Therefore, the moles of oxygen consumed can be calculated as:
(5/1) * 0.612 mol = 3.06 mol
4. Calculate the molar mass of carbon dioxide (CO2). Carbon has a molar mass of 12.01 g/mol, and oxygen has a molar mass of 16.00 g/mol. Therefore, the molar mass of carbon dioxide is:
(12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol
5. Finally, calculate the grams of carbon dioxide produced by multiplying the molar mass of carbon dioxide with the moles of carbon dioxide:
44.01 g/mol * 0.612 mol = 26.95 g
Therefore, approximately 26.95 grams of carbon dioxide can be produced from the given reactants.
To find out how many grams of carbon dioxide can be made, we need to use the concept of stoichiometry. Stoichiometry involves using the balanced chemical equation and applying the mole ratio to determine the quantities of reactants and products involved in a chemical reaction.
The balanced chemical equation for the combustion of propane is:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
We can use this equation to determine the number of moles of carbon dioxide produced from the given amount of propane.
First, we need to convert the mass of propane into moles. To do this, we divide the given mass (27 grams) by the molar mass of propane (44.1 g/mol). This gives us:
27 g / 44.1 g/mol = 0.613 mol
According to the balanced equation, each mole of propane reacts to produce 3 moles of carbon dioxide. Therefore, we can multiply the number of moles of propane by the mole ratio to find the number of moles of carbon dioxide produced:
0.613 mol C₃H₈ x (3 mol CO₂ / 1 mol C₃H₈) = 1.839 mol CO₂
Finally, we need to convert the number of moles of carbon dioxide into grams. The molar mass of carbon dioxide (CO₂) is approximately 44.0 g/mol. So, we multiply the number of moles of carbon dioxide by its molar mass:
1.839 mol CO₂ x 44.0 g/mol = 80.916 g CO₂
Therefore, approximately 80.9 grams of carbon dioxide can be produced from the given amounts of propane and oxygen.