I did this in school and you should search the title in google and it will appear that what I did and it worked good luck
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]
Excess silicon dioxide" tells us carbon is the limiting reactant, and thus the amount of silicon carbide produced depends on how much carbon is available to react.
*Based on the balanced equation, for every 3 moles carbon reacted, 1 mole silicon carbide is produced.
*Molar mass carbon: 12.01 g/mol
*Molar mass silicon carbide: 28.09 g + 12.01 g = 40.1 g/mol
79.1 g carbon x (1 mol carbon / 12.01 g carbon) x (1 mol silicon carbide / 3 mol carbon) x (40.1 g silicon carbide / 1 mol silicon carbide) = 88.04 g silicon carbide
