How many moles of H2O (g) are produced when 4.3 grams O2 (g) are consumed?
C4H6+O2-->CO2+H2O
My try at balance is:
C4H6+4O2+3/2O2-->4CO2+3H2O
Well, it seems like you're trying to balance the chemical equation there... but it looks like you've got one too many oxygens on the left side. Let me give it a shot:
C4H6 + 9O2 → 4CO2 + 6H2O
Now that the equation is balanced, we can see that for every 6 moles of water produced, 9 moles of oxygen are consumed. So, if 4.3 grams of oxygen (O2) are consumed, we'll need to do a little math to find out how many moles of water are produced.
First, we need to calculate the molar mass of oxygen (O2). The molar mass of O2 is approximately 32 grams/mol.
Now, using the molar mass of O2, we can calculate the number of moles:
moles O2 = mass / molar mass
moles O2 = 4.3 g / 32 g/mol ≈ 0.134 moles
Since the stoichiometric ratio between oxygen (O2) and water (H2O) is 9:6, we can set up a proportion to find the number of moles of water (H2O):
9 moles O2 = 6 moles H2O
0.134 moles O2 = x moles H2O
Cross-multiplying, we find:
x ≈ (0.134 moles H2O * 6 moles H2O) / 9 moles O2
x ≈ 0.089 moles H2O
So, approximately 0.089 moles of water (H2O) are produced when 4.3 grams of oxygen (O2) are consumed.
To determine the number of moles of H2O (g) produced, we first need to balance the chemical equation correctly. Here is the balanced equation:
C4H6 + 6O2 → 4CO2 + 3H2O
Now, let's calculate the number of moles of H2O produced when 4.3 grams of O2 are consumed.
Step 1: Convert the mass of O2 to moles.
To do this, we need to know the molar mass of O2, which is 32 g/mol.
moles of O2 = mass of O2 / molar mass of O2
moles of O2 = 4.3 g / 32 g/mol
moles of O2 ≈ 0.1344 mol
Step 2: Determine the mole ratio between O2 and H2O.
From the balanced equation, we can see that the mole ratio between O2 and H2O is 6:3 (or 2:1).
Step 3: Calculate the number of moles of H2O.
We can now use the mole ratio to determine the number of moles of H2O produced.
moles of H2O = moles of O2 × (moles of H2O / moles of O2)
moles of H2O = 0.1344 mol × (3 mol H2O / 6 mol O2)
moles of H2O ≈ 0.0672 mol
Therefore, approximately 0.0672 moles of H2O (g) are produced when 4.3 grams of O2 (g) are consumed.
To determine the number of moles of H2O (g) produced when 4.3 grams of O2 (g) are consumed, you need to follow these steps:
1. Determine the molar mass of O2 (g). Oxygen (O) has a molar mass of approximately 16.00 g/mol. Since there are two oxygen atoms in O2, the molar mass of O2 is 2 * 16.00 = 32.00 g/mol.
2. Calculate the number of moles of O2 by dividing the given mass (4.3 grams) by the molar mass of O2: 4.3 g / 32.00 g/mol = 0.1344 mol.
3. Now let's use the balanced chemical equation you provided where 4 moles of CO2 are produced for every 3 moles of H2O.
Based on the provided equation:
C4H6 + 4O2 + (3/2)O2 -> 4CO2 + 3H2O
4. To determine the moles of H2O formed, you need to know the moles of O2 consumed. From step 2, we know there are 0.1344 mol of O2.
Since the stoichiometric coefficient for H2O in the balanced equation is 3, we need to multiply the moles of O2 by the molar ratio between O2 and H2O. In this case, the ratio is 3 moles of H2O per 4 moles of O2.
Therefore, the moles of H2O formed can be calculated as: 0.1344 mol O2 * (3 moles H2O / 4 moles O2) = 0.1008 mol H2O.
So, when 4.3 grams of O2 are consumed, approximately 0.1008 moles of H2O are produced.
You have it balanced but it is awkward. It makes things easier to use whole numbers.
2C4H6 + 11O2 ==> 8CO2 + 6H2O
Here is a site that gives a worked example of how to solve a stoichiometry problem (which this is).
http://www.jiskha.com/science/chemistry/stoichiometry.html