Answer: 11.2 moles of 
are produced when 5.60 mol of ethane is burned in an excess of oxygen.
Explanation:
The combustion of ethane is represented using balanced chemical equation:
As oxygen is preset in excess, ethane acts as the limiting reagent as it limits the formation of product.
According to stoichiometry :
2 moles of propane produces 4 moles of carbon dioxide
Thus 5.60 moles of propane will produce=
moles of carbon dioxide
Thus 11.2 moles of are produced when 5.60 mol of ethane is burned in an excess of oxygen.
Answer:
3 Cu + 8 HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O
Explanation:
Make sure both sides are equal
3 <u>Cu</u> + 8 H<u>N</u>O3 --> 3 <u>Cu</u>(NO3)2 + 2 <u>N</u>O + 4 H2O
// start by those elements that change their oxidation degree
<u>Cu</u> and <u>N</u>
// also you can write reduction-oxidation reactions
+ 2 
--> 
| 2
- 3 --> 
| 3
// write the numbers of electrons that are lost/gained as the coefficients of the opposite elements
// then check if H and O are the same on both sides
// adjust if they aren't.
The two Amino Acids drawn are;
1) Proline (Red)
2) Histidine (Blue)
The <em>Carboxylic Groups </em>are encircled in Yellow Sphere.
The <em>Amino Groups</em> are encircled in Orange Spheres.
The <em>Alpha carbons</em> are encircled in Pink spheres.
The <em>water molecule</em> evolved is in corresponding colors of its parent molecules.
The<em> peptide bond</em> formed is colored by Green color.
The total pressure of the mixture of gases is equal to the sum of the pressure of each gas as if it is alone in the container. The partial pressure of a component of the mixture is said to be equal to the product of the total pressure and the mole fraction of the component in the mixture.
Partial pressure of hydrogen gas = 1.24 atm x .25 = 0.31 atm
Partial pressure of the remaining = 1.24 atm x (1-.25) = 0.93 atm
