Ahh the charges! I know just how to help!!
One thing I do is I draw each individual proton or electron out. Make sure you label each proton with a + and each electron with a -.
Then I cross them out. For each proton you cross out, cross out an electron and vice-versa.
If you end with a proton, then the atom is positive.
If you end with an electron, then the atom is negative.
If you end with nothing, then it is neutral.
HOPE THIS HELPS!!!!!! Let me know if you have more questions!!
Answer:
Lowering activation energy of a reaction.
Explanation:
Activation energy is the minimum amount of energy required by the reactants just to be converted to products.
Since catalysts increase the rate of reaction, activation complex is reached in short period of time hence activation energy is lowered.
d. sulphur
Because sulphur, once it escapes into the atmosphere can cause acid rain.
Answer:
Answers are in the explanation.
Explanation:
- The half‑life of A increases as the initial concentration of A decreases. order: <em>2. </em>In the half-life of second-order reactions, the half-life is inversely proportional to initial concentration.
- A three‑fold increase in the initial concentration of A leads to a nine‑fold increase in the initial rate. order: <em>2. </em>The rate law of second-order is: rate = k[A]²
- A three‑fold increase in the initial concentration of A leads to a 1.73‑fold increase in the initial rate. order: <em>1/2. </em>The rate law for this reaction is: rate = k √[A]
- The time required for [A] to decrease from [A]₀ to [A]₀/2 is equal to the time required for [A] to decrease from [A]₀/2 to [A]₀/4. order: <em>1. </em>The concentration-time equation for first-order reaction is: ln[A] = ln[A]₀ - kt. That means the [A] decreasing logarithmically.
- The rate of decrease of [A] is a constant. order: <em>0. </em>The rate law is: rate = k -<em>where k is a constant-</em>