Answer:
Chemicals are used in the manufacturing of fertilizers
Answer:
1.5
Explanation:
Given that :
Compound A and B are formed from Sulfur + Oxygen.
Compound A :
6g sulfur + 5.99g Oxygen
Compound B:
8.6g sulfur + 12.88g oxygen
Comparing the ratios :
Compound A:
S : O = 6.00 : 5.99
S/0 = 6.0g S / 5.99g O
Compound B :
S : O = 8.60 : 12.88
S / O = 8.60g S / 12.88g O
Mass Ratio of A / mass Ratio of B
(6.0g S / 5.99g O) ÷ (8.60g S / 12.88g O)
(6.0 g S / 5.99g O) × (12.88g O / 8.60g S)
(6 × 12.88) / (5.99 × 8.60)
= 77.28 / 51.514
= 1.50017
= 1.5
Explanation:
Removing B from the system
- Decreases the rate of the reaction. Backward reaction (formation of reactants) is favoured.
Crushing A into a powder
- Increases the rate of reaction. This is because of the increased surface area of A.
Warming the system
- Increases the rate of the reaction. Temperature is proportional to rate of reaction.
Adding more A to the system
- Increases the rate of reaction. Forward reaction (formation of products) is favoured.
Putting the system into an ice bath
- Decreases the rate of reaction. Temperature is proportional to rate of reaction.
Decreasing the pressure of the system
- Decreases the rate of the reaction.
Answer:
Rate = 43 M⁻¹s⁻¹[NO₂][O₃]
Explanation:
We need to find the reaction order in
rate = (NO₂ )ᵃ (O₃ )ᵇ
given:
( NO₂ ) M ( O₃ ) M Rate M/s
0.10 0.33 1.420 (1)
0.10 0.66 2.840 (2)
0.25 0.66 7.10 (3)
When keeping the NO₂ concentration constant in the first two while doubling the concentration of O₃ , the rate doubles. Therefore it is first order with respect to O₃
Comparing (2) and (3) increasing the concentration of NO₂ by a factor of 2.5 and keeping O₃ constant , increased the rate by a factor of 2.5. Therefore the rate is first order with respect to NO₂
Then rate law is
= k (NO₂) (O₃ )
To find k take any of the three and substitute the values to find k:
1.420 M/s = k (0.10)M x (0.33)M ⇒ k = 43 /Ms
Then the answer is Rate = 43 M⁻¹s⁻¹[NO₂][O₃]
