Answer:
k = 2.647 x 10-2 M-2 s-1
Explanation:
2NO(g) +Cl2(g) --> 2NOCl(g)
Experiment [NO] (M) [Cl2] (M) Rate (M/s)
1 0.0300 0.0100 3.4 x 10-4
2 0.0150 0.0100 8.5 x 10-5
3 0.0150 0.0400 3.4 x 10-4
Frrom experiments 1 and 3;
Reducing the concentration of NO by a factor of 2 decreases the rate of the reaction by a factor of 4. This means the reaction is second order with respect to NO.
From experiments 2 and 3:
Increasing the concentration of Cl2 by a factor of 4 increases the rate by a factor of 4. This means the reaction is first order with respect to Cl2
The rate equation is given as;
Rate = k [NO]² [Cl2]
From experiment 1;
k = [NO]² [Cl2] / Rate
k = 0.0300² * 0.0100 / 3.4 x 10-4
k = 2.647 x 10-2 M-2 s-1
The correct answer is (C. zirconium - 93.
<h3>
Answer:</h3>
45°C
<h3>
Explanation:</h3>
We are given;
- Quantity of heat = 1.95 kJ
- Mass of lead = 500 g
- Initial temperature = 15° C
- heat capacity of lead is 130 J/kg°C
We are required to calculate the final temperature;
- We need to know that the quantity of heat is given by the formula;
Q = mass,m × specific heat,c × Change in temperature,ΔT
ΔT = final temperature - initial temperature
We can rearrange the formula to calculate the change in temperature
ΔT = Q ÷ (m×c)
Therefore;
ΔT = 1950 J ÷ (0.5 kg × 130 J/Kg°C)
= 30°C
But,
Final temperature = ΔT + Initial temperature
= 15°C + 30°C
= 45°C
Therefore, the final temperature is 45°C