Answer:
N₂ = 0.7515atm
O₂ = 0.1715atm
NO = 0.0770atm
Explanation:
For the reaction:
N₂(g) + O₂(g) ⇄ 2NO(g)
Where Kp is defined as:
Pressures in equilibrium are:
N₂ = 0.790atm - X
O₂ = 0.210atm - X
NO = 2X
Replacing in Kp:
0.0460 = [2X]² / [0.790atm - X] [0.210atm - X]
0.0460 = 4X² / 0.1659 - X + X²
0.0460X² - 0.0460X + 7.6314x10⁻³ = 4X²
-3.954X² - 0.0460X + 7.6314x10⁻³ = 0
Solving for X:
X = - 0.050 → False answer. There is no negative concentrations.
X = <em>0.0385 atm</em> → Right answer.
Replacing for pressures in equilibrium:
N₂ = 0.790atm - X = <em>0.7515atm</em>
O₂ = 0.210atm - X = <em>0.1715atm</em>
NO = 2X = <em>0.0770atm</em>
The statement is false because endothermic reactions have a positive enthalpy change, because heat is being added to the system because it requires more energy to react
Explanation:
2H2+O2------->2H2O
its yr balanced equation.
hope it helps
<h2>stay safe healthy and happy....</h2>
Answer:
3.72L
Explanation:
Given parameters:
Initial volume V₁ = 3.9L
Condition = STP
Final temperature T₂ = -550°C
Final pressure P₂ = 880mmHg
Unknown:
Final volume V₂ = ?
Solution.
At standard temperature and pressure(STP), the:
Pressure = 1atm = 760mmHg
Temperature = 273K
Therefore, P₁ = 760mmHg
T₁ = 273K
The general gas law, is best to solve this problem. It is mathematically given as:
Let us take the units to the appropriate one;
-550°C = 273 + (-550) = -277K
Input the variables;
V₂ = 3.72L
