Explanation:
Question 1
Rate constant = 3.50×10−3 s−1
Initial Concentration [A]o = 0.450 M
Final concentration [A] = ?
time = 19 minutes = 1140 s (upon conversion to seconds)
Integrated rate law for a first order reaction is given as;
ln[A] = ln[A]o - kt
ln[A] = ln (0.450) - (3.50×10−3)1140
ln[A] = -0.799 - 3.99
ln[A] = -4.789
[A] = 0.0083M
Question 2
Rate constant, k = 3.50×10−4 M/s
time = 65 s
Final Concentration [A] = 3.50×10−2 M
Initial Concentration [A]o = ?
Integrated rate law for a first order reaction is given as;
[A] = [A]o - kt
[A]o = [A] + kt
[A]o = 3.50×10−2 + (3.50×10−4) * 65
[A]o = 3.50×10−2 + 0.02275
[A]o = 0.05775 M
Answer:
They also showed the effects of pressure on volume if temperature stayed the same
Explanation:
They also showed the effects of pressure on volume if temperature stayed the same is the experiment that will provide an evidence for Boyle's law.
Boyle's law states that "the volume of a fixed mass of a gas varies inversely as the pressure changes, if the temperature is constant".
- The law is an affirmation of what happens when there is a dynamics between pressure and volume if temperature is made constant.
- So the experiment designed to investigate this proves and shows Boyle's law.
I don't understand the elements, which ones are capital letters and which ones are lower case.
Answer:
a) equilibrium shifts towards the right
b) equilibrium shifts towards the right
c) equilibrium shifts towards the left
d) has no effect on equilibrium position
e) has no effect on equilibrium position
Explanation:
A reversible reaction may attain equilibrium in a closed system. A chemical system is said to be in a state of dynamic equilibrium when the rate of forward reaction is equal to the rate of reaction.
According to Le Chateliers principle, when a constraint such as a change in temperature, pressure, volume or concentration is imposed upon a system in equilibrium, the equilibrium position shifts in such a way as to annul the constraint.
When the concentration of reactants is increased, the equilibrium position is shifted towards the right hand side and more products are formed. For an endothermic reaction, the reverse reaction is favoured by a decrease in temperature. Increase in pressure has no effect on the system since there are equal volumes on both sides of the reaction equation. Similarly, the addition of a catalyst has no effect on the equilibrium position since it speeds up both the forward and reverse reactions to the same extent.