Answer:
Explanation:
<u>1) Rate law, at a given temperature:</u>
- Since all the data are obtained at the same temperature, the equilibrium constant is the same.
- Since only reactants A and B participate in the reaction, you assume that the form of the rate law is:
r = K [A]ᵃ [B]ᵇ
<u>2) Use the data from the table</u>
- Since the first and second set of data have the same concentration of the reactant A, you can use them to find the exponent b:
r₁ = (1.50)ᵃ (1.50)ᵇ = 2.50 × 10⁻¹ M/s
r₂ = (1.50)ᵃ (2.50)ᵇ = 2.50 × 10⁻¹ M/s
Divide r₂ by r₁: [ 2.50 / 1.50] ᵇ = 1 ⇒ b = 0
- Use the first and second set of data to find the exponent a:
r₁ = (1.50)ᵃ (1.50)ᵇ = 2.50 × 10⁻¹ M/s
r₃ = (3.00)ᵃ (1.50)ᵇ = 5.00 × 10⁻¹ M/s
Divide r₃ by r₂: [3.00 / 1.50]ᵃ = [5.00 / 2.50]
2ᵃ = 2 ⇒ a = 1
<u>3) Write the rate law</u>
This means, that the rate is independent of reactant B and is of first order respect reactant A.
<u>4) Use any set of data to find K</u>
With the first set of data
- r = K (1.50 M) = 2.50 × 10⁻¹ M/s ⇒ K = 0.250 M/s / 1.50 M = 0.167 s⁻¹
Result: the rate constant is K = 0.167 s⁻¹
<u>Answer:</u> The final volume will be 14.85 L.
<u>Explanation:</u>
To calculate the final volume when temperature increases, we use Charles' Law.
This law states that volume is directly proportional to the temperature of the gas if number of moles and pressure remains constant.
where,
= Initial volume and temperature
= Final volume and temperature
We are given:
Putting values in above equation, we get:
Hence, the final volume of the gas is 14.85L
Answer:
Explanation:
To solve this problem, we can use the Combined Gas Laws:
Data:
p₁ = 2.02 atm; V₁ = 736 mL; n₁ = n₁; T₁ = 1 °C
p₂ = ?; V₂ = 416 mL; n₂ = n₁; T₂ = 82 °C
Calculations:
(a) Convert the temperatures to kelvins
T₁ = ( 1 + 273.15) K = 274.15 K
T₂ = (82 + 273.15) K = 355.15 K
(b) Calculate the new pressure
