Answer:
10.07 L is the volume for the produced N₂
Explanation:
This is a question for the Ideal Gases Equation:
P . V = n . R . T
In STP conditions, the pressure is 1 atm and the T° is 273K
Let's determine the moles of produced N₂ by the decomposition of TNT
The reaction is:
2 C₇H₅(NO₂)₃ (s) → 7 C (s) + 7 CO (g) + 3 N₂ (g) + 5 H₂O (g)
We convert the mass to moles (mass / molar mass)
68.2 g . 1 mol / 227.13 g = 0.300 moles
Ratio is 2:3. 2 moles of TNT can produce 3 moles of N₂
Then, 0.300 moles will produce (0.300 . 3) / 2 = 0.450 moles
We replace data:
1 atm . V = 0.450 mol . 0.082 L.atm/mol.K . 273K
V = (0.450 mol . 0.082 L.atm/mol.K . 273K) / 1 atm
V = 10.07 L
Answer:
1.005 cm³
Explanation:
Using Ideal gas equation for same mole of gas as
Given ,
V₁ = 0.650 cm³
V₂ = ?
P₁ = 1.54 atm
P₂ = 1.01 atm
T₁ = 12°C
T₂ = 16 ºC
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (12 + 273.15) K = 285.15 K
T₂ = (16 + 273.15) K = 289.15 K
Using above equation as:
Solving for V₂ , we get:
<u>V₂ = 1.005 cm³</u>
I’m really sorry I need points I hope you find an answer
Answer:
1) B. increases
2) B. greater
3) C. Both A and B are correct
4) Activation energy
Explanation:
The rate of a chemical reaction is depend on temperature. If temperature increases, the chemical reaction also increases and vice versa. Fast reaction means which is completely in less time. So atoms in fast reaction have great activation energy and slow reaction have less activation energy. Collision occurs when the particles have energy to move and they collide in proper direction.
