Answer:
Hi I think that its oats.
Explanation: It has fiber and vitamin c
 
        
                    
             
        
        
        
You need to use Stoichiometry
 
        
             
        
        
        
Answer:
<em />
<em>a) Balanced chemical equation:</em>
<em />
<em>       </em> <em />
<em />
<em />
<em>b) Theoretical yield:</em>
c) % yield:
Explanation:
The complete question is:
<em>In a particular reaction 6.80g of dinitrogen trioxide gas (N₂0₃) was actually produced by reacting 8.75g of oxygen gas (O₂) with excess nitrogen gas (N₂)</em>
<em>a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation.</em>
<em>b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis</em>
<em>c) Calculate the % yield of the product</em>
<em />
<h2>Solution</h2>
<em />
<em>a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation.</em>
<em />
<em>       </em> <em />
<em />
<em />
Check the balance:
<em />
Atom     Left-handside    Right-hand side
   N              2×2=4                  2×2=4
   O              3×2=6                  2×3=6
- Mole ratio: it is the ratio of the coefficients of the balanced equation
         
<em>b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis</em>
<em />
<u>1. Convert 8.75 g of O₂(g) to number of moles</u>
- number of moles = mass in grams / molar mass
- molar mass of O₂ = 15.999g/mol
- number of moles = 8.75g / 15.999 g/mol = 0.5469 mol O₂
<u />
<u>2. Use dimensional analysis to calculate the maximum number of moles of N₂O₃(g) that can be produced</u>
       
<u>3. Convert to mass in grams</u>
- mass = number of moles × molar mass
- molar mass of N₂O3 = 76.01g/mol
- mass = 0.3646mol × 76.01g/mol = 27.7g N₂O3
<em>c) Calculate the % yield of the product</em>
<em />
Formula:
<em />
- %yield = (actual yield/theoretical yield)×100
Substitute and compute:
- % yield = (6.80g/27.7g)×100 = 24.5% 
<em />