Refer to the following equation: 4NH3 + 7O2= 4NO2 +6HO, How many moles of ammonia would be required to produce 11.9 mol of water?
Can you please walk me through the steps on how to figure this problem?
7.93 mol
It's an easy walk through the park. Use the coefficients in the balanced equation and dimensional analysis.
11.9 mols H2O x (4 mols NH3/6 mol H2O) = 11.9 x (4/6) = ? mols NH3 required.
Well, determining the number of moles of ammonia required to produce 11.9 mol of water is actually quite simple!
First, let's look at the balanced chemical equation: 4NH3 + 7O2 = 4NO2 + 6H2O. From this equation, we can see that for every 6 moles of water produced, we need 4 moles of ammonia.
So, using a simple proportion, we can set up the equation:
(4 moles of ammonia) / (6 moles of water) = (x moles of ammonia) / (11.9 moles of water)
Now, let's solve for x:
Cross-multiplying:
6 moles of water * x moles of ammonia = 4 moles of ammonia * 11.9 moles of water
Rearranging the equation:
x = (4 moles of ammonia * 11.9 moles of water) / 6 moles of water
Calculating the result:
x = 47.6 moles of ammonia / 6 moles of water
Simplifying the ratio:
x ≈ 7.93 moles of ammonia
So, approximately 7.93 moles of ammonia are required to produce 11.9 mol of water.
Hope that makes you happier than a clown with a balloon animal!
To find out how many moles of ammonia are needed to produce 11.9 mol of water, we need to use the balanced chemical equation and the given coefficient ratios.
The balanced chemical equation is: 4NH3 + 7O2 = 4NO2 + 6H2O.
Comparing the coefficients of ammonia (NH3) and water (H2O) in the equation, we see that the ratio is 4:6. This means that for every 4 moles of ammonia, 6 moles of water are produced.
We can set up a proportion to find the number of moles of ammonia required:
4 moles NH3 / 6 moles H2O = x moles NH3 / 11.9 moles H2O.
Cross-multiplying, we get:
6 * x = 4 * 11.9.
Simplifying, we have:
6x = 47.6.
Dividing both sides by 6:
x = 7.93.
Therefore, approximately 7.93 moles of ammonia are required to produce 11.9 moles of water.
To figure out how many moles of ammonia would be required to produce 11.9 mol of water, we need to use the balanced equation and the concept of stoichiometry.
First, let's examine the balanced equation:
4NH3 + 7O2 -> 4NO2 + 6H2O
From the equation, we can see that for every 4 moles of NH3 (ammonia), we produce 6 moles of H2O (water).
To calculate the amount of ammonia needed to produce 11.9 mol of water, we can set up a proportion based on the stoichiometry of the equation:
4 moles NH3 / 6 moles H2O = x moles NH3 / 11.9 moles H2O
Simplifying the proportion:
(4/6) = (x/11.9)
Cross-multiplying:
6x = 4 * 11.9
6x = 47.6
Dividing both sides by 6:
x = 47.6 / 6
x ≈ 7.933
Therefore, approximately 7.933 moles of ammonia would be required to produce 11.9 mol of water.