Explanation:
Charges on both magnesium and oxygen is 2. Though opposite in sign, they have equal charges so, both of them will be cancelled by each other.
As a result, formula of magnesium oxide is MgO and not 
.
The student write the equation as 
, it is not correct.
Therefore, given equation will be balanced as follows.
Since, number of atoms on both reactant and product side are equal. Hence, this equation is completely balanced.
The balanced chemical
reaction will be:
2H2O = 2H2 + O2
<span>We are given the amount of water used in the decomposition reaction. This will be our
starting point.</span>
<span>17.0 g H2O</span> (1 mol H2O/ 18.02 g H2O) (1 mol O2/2
mol <span>H2O</span>) ( 32.00 g O2/1mol O2) = 15.09 g O2
Percent yield = actual yield / theoretical yield x 100
<span>Percent yield =10.2 g / 15.09 g
x 100</span>
Percent yield = 67.58%
It allows you to determine the relation between the reactants and the products.
<h3><u>Answer;</u></h3>
= 3032.15 kPa
<h3><u>Explanation;</u></h3>
Using the equation;
PV = nRT , where P is the pressure,. V is the volume, n is the number of moles and T is the temperature and R is the gas constant, 0.08206 L. atm. mol−1.
Volume = 7.5 L, T = 274 +273 = 547 K, N = 5 moles
Therefore;
Pressure = nRT/V
= (5 × 0.08206 × 547)/7.5 L
= 29.925 atm
But; 1 atm = 101325 pascals
Hence; Pressure = 3032150.63 pascals
<u>= 3032.15 kPa</u>
Answer:
8.0 mol O₂
Explanation:
Let's consider the complete combustion reaction of C₉H₁₂.
C₉H₁₂ + 12 O₂ → 9 CO₂ + 6 H₂O
The molar ratio of C₉H₁₂ to O₂ is 1:12. The moles of O₂ required to react with 0.67 moles of C₉H₁₂ are:
0.67 mol C₉H₁₂ × (12 mol O₂/1 mol C₉H₁₂) = 8.0 mol O₂
8.0 moles of O₂ are required to completely react with 0.67 moles of C₉H₁₂.
