I'll balance it for you :D
HNO3 + P → <span>H3PO4 + NO
break it down first (to see how many of each atom on each side) so
H- 1 H-3
N-1 N-1
O-3 O-12
P-1 P-3
now u gotta make the numbers equal on both sides
make the first H 3 so it's balanced with the other one by putting a 3 in front of it in the equation like this:
</span>3HNO3 + P → H3PO4 + NO
<span>
that changes the WHOLE equation except the P because it's not attached (so now the N is also 3 and the O as well)
</span>H- 3 H-3
N-3 N-1
O-9 O-12
P-1 P-3
so now the N is imbalanced on the product side, so do the same thing to fix it
3HNO3 + P → H3PO4 + 3NO
the O next to the N is now also 3 sooo
H- 3 H-3
N-3 N-3
O-9 O-15
P-1 P-3
3HNO3 + 3P → H3PO4 + 3NO
H- 3 H-3
N-3 N-3
O-9 O-15
P-3 P-3
3HNO3 + 3P → H3PO4 + 3NO
i realized halfway through this that the O is still unbalanced SOMEHOW
Salt!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
Answer:
A. Energy is necessary for bond formation.
C. Breaking bonds takes energy.
D. When bonds are formed, energy is released.
Energy is always required for bond formation because when a chemical reaction occurs, either molecular bonds are broken or other bonds are formed to make different molecules. Energy is released during bond formation and is an exothermic process because bond formation represents a stable configuration and the energy lost is released as heat energy that makes it more stable. Breaking bonds takes energy and is an endothermic reaction because energy is absorbed to break bonds.
Hope that helps. x
Answer:
0.59 moles
Explanation:
Data Given
oxygen = 35 g
Moles of SeO₃ = ?
Reaction Given
2Se + 3O₂ ------> 2SeO₃
Solution:
Step 1.
First to find grams of SeO₃
So, we know from reaction that 2 mole of selenium combine with 3 mole of oxygen and produces 2 mole of SeO₃
2Se + 3O₂ ------> 2SeO₃
2mol 3 mol 2 mol
If we represent mole in grams
Then,
Molar mass of Se = 79 g/mol
Molar mass of O = 16 g/mol
Molar mass of SeO₃ = 79 + 3(16)
Molar mass of SeO₃ = 127 g/mol
2Se + 3O₂ ------> 2SeO₃
2mol (79 g/mol) 3 mol (32 g/mol) 2 mol (127 g/mol)
2Se + 3O₂ ------> 2SeO₃
158 g 96 g 206 g
It is obvious from the reaction that 96 g of oxygen gives 206 g of SeO₃.
Now how many grams of SeO₃ will produce if 35 grams of oxygen react with excess of Selenium
Apply unity formula
96 g of O₂ ≅ 206 g of SeO₃
35 g of O₂ ≅ x g of SeO₃
By doing cross multiplication
g of SeO₃ = 206 x 35 / 96
g of SeO₃ = 75 g
Step 2.
Convert grams of SeO₃ to mole
Formula used
no. of moles = mass in grams (SeO₃) / Molar mass of SeO₃
Put values in above formula
no. of moles = 75 g / 127 g/mol
no. of moles = 0.59 mol
So,
35 g of oxygen produces 0.59 moles of SeO₃