A catalytic converter combines 2.55 g CO with excess O2.What mass of CO2 forms?
Well, I guess that depends on how persuasive the catalytic converter is at getting the CO and O2 to bond. Do they have a good chemistry? Do they exchange lovely electrons? Are they the perfect match made in chemical heaven? If so, then I'm willing to bet they'll produce quite a bit of CO2.
To determine the mass of CO2 that forms when 2.55 g of CO reacts with excess O2, we first need to balance the equation for the reaction:
2 CO + O2 → 2 CO2
From the balanced equation, we can see that 2 moles of CO react with 1 mole of O2 to produce 2 moles of CO2. We can use this information to calculate the moles of CO2 formed.
1. Convert the mass of CO to moles:
Molar mass of CO = 28.01 g/mol
Moles of CO = mass of CO / molar mass of CO
= 2.55 g / 28.01 g/mol
2. Use the mole ratio from the balanced equation to determine the moles of CO2 formed:
Moles of CO2 = Moles of CO * (2 moles of CO2 / 2 moles of CO)
= (2.55 g / 28.01 g/mol) * (2/2)
= 0.1815 mol
3. Convert the moles of CO2 to mass:
Molar mass of CO2 = 44.01 g/mol
Mass of CO2 = Moles of CO2 * molar mass of CO2
= 0.1815 mol * 44.01 g/mol
= 7.999 mol
Therefore, the mass of CO2 formed is approximately 8.0 g.
To determine the mass of CO2 formed when 2.55 g of CO reacts with excess O2, we need to first balance the chemical equation for the reaction.
The balanced equation for the reaction between CO and O2 to form CO2 is:
2 CO + O2 -> 2 CO2
According to the balanced equation, 2 moles of CO react with 1 mole of O2 to produce 2 moles of CO2.
To solve this problem, we will follow these steps:
Step 1: Convert the given mass of CO to moles.
Step 2: Use the mole ratio from the balanced equation to determine the number of moles of CO2 formed.
Step 3: Convert the moles of CO2 to grams.
Step 1: Convert the given mass of CO to moles.
The molar mass of CO is the sum of the atomic masses of carbon (C) and oxygen (O):
Molar mass of CO = 12.01 g/mol (atomic mass of carbon) + 16.00 g/mol (atomic mass of oxygen) = 28.01 g/mol
To obtain moles, we will use the formula:
moles = mass / molar mass
moles of CO = 2.55 g / 28.01 g/mol = 0.0911 mol
Step 2: Use the mole ratio from the balanced equation to determine the number of moles of CO2 formed.
According to the balanced equation, 2 moles of CO react to produce 2 moles of CO2.
moles of CO2 = moles of CO (since the mole ratio is 1:1) = 0.0911 mol
Step 3: Convert the moles of CO2 to grams.
The molar mass of CO2 is the sum of the atomic masses of carbon (C) and two oxygen (O) atoms:
Molar mass of CO2 = 12.01 g/mol (atomic mass of carbon) + 2 * 16.00 g/mol (atomic mass of oxygen) = 44.01 g/mol
To obtain grams, we will use the same formula as in Step 1:
mass = moles x molar mass
mass of CO2 = 0.0911 mol x 44.01 g/mol = 4.004 g
Therefore, the mass of CO2 formed is approximately 4.004 grams.
Here is a sample stoichiometry problem worked. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html