If 150.0 g of butane (C4H10) gas are burned, how many grams of carbon dioxide gas will be produced? Report your answer to the nearest whole number and do not include units in your answer.
Do not use scientific notation for your answer.
This is a stoichiometry problem.
Write an balance the equation.
Convert 150.0 g butane to mols. mols = grams/molar mass
Using the coefficients in the balanced equation, convert mols butane to mols CO2.
Then g CO2 = mols CO2 x molar mass CO2.
Determine how many grams of CO2 are produced by burning 1.01 g of C4H10.
To solve this stoichiometry problem, we need to use the balanced chemical equation for the combustion of butane (C4H10):
2 C4H10 + 13 O2 → 8 CO2 + 10 H2O
According to the equation, 2 moles of butane react with 13 moles of oxygen gas to produce 8 moles of carbon dioxide gas.
First, we need to convert the given mass of butane to moles using its molar mass of 58.12 g/mol:
150.0 g C4H10 × (1 mol C4H10/58.12 g C4H10) = 2.583 mol C4H10
Next, we use the mole ratio from the balanced equation to determine the moles of carbon dioxide produced:
2.583 mol C4H10 × (8 mol CO2/2 mol C4H10) = 10.332 mol CO2
Finally, we convert the moles of carbon dioxide to grams using its molar mass of 44.01 g/mol:
10.332 mol CO2 × (44.01 g CO2/1 mol CO2) = 454.7 g CO2
Rounding to the nearest whole number, the mass of carbon dioxide produced is 455 g.
To solve this stoichiometry problem, we need to use the balanced chemical equation for the combustion of butane. The balanced equation is:
2C4H10 + 13O2 -> 8CO2 + 10H2O
From the equation, we can see that 2 moles of butane react to produce 8 moles of carbon dioxide. We need to convert the given mass of butane to moles using its molar mass and then use the mole ratio to find the moles of carbon dioxide produced. Finally, we can convert the moles of carbon dioxide to grams using its molar mass.
1. Calculate the moles of butane:
molar mass of butane (C4H10) = 12.01 g/mol (carbon) + 4 * 1.01 g/mol (hydrogen) = 58.12 g/mol
moles of butane = mass of butane / molar mass of butane = 150.0 g / 58.12 g/mol = 2.58 mol (rounded to two decimal places)
2. Use the mole ratio to determine moles of carbon dioxide:
moles of butane : moles of carbon dioxide = 2 : 8
moles of carbon dioxide = (2.58 mol butane) * (8 mol CO2 / 2 mol butane) = 10.32 mol (rounded to two decimal places)
3. Calculate the mass of carbon dioxide:
molar mass of carbon dioxide (CO2) = 12.01 g/mol (carbon) + 2 * 16.00 g/mol (oxygen) = 44.01 g/mol
mass of carbon dioxide = moles of carbon dioxide * molar mass of carbon dioxide = 10.32 mol * 44.01 g/mol = 454 g (rounded to the nearest whole number)
Therefore, approximately 454 grams of carbon dioxide gas will be produced.