Answer:
1) Increasing the pressure C) Shift to the right
2) Removing hydrogen gas A) Shift to the left
3) Adding a catalyst B) No effect
Explanation:
- <em>Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.</em>
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<u><em>1) Increasing the pressure:</em></u>
- When there is an increase in pressure, the equilibrium will shift towards the side with fewer moles of gas of the reaction. And when there is a decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.
- The reactants side (left) has 4.0 moles of gases and the products side (right) has 2.0 moles of gases.
- So, increasing the pressure will shift the reaction to the side with lower moles of gas (right side).
- <u><em>so, the right match is: C) Shift to the right.</em></u>
<em><u>2) Removing hydrogen gas:</u></em>
- Removing hydrogen gas will decrease the concentration of the products side, so the reaction will be shifted to the lift side to suppress the decrease in the concentration of hydrogen gas by removing.
- <em>so, the right match is: A) Shift to the left.</em>
<u><em>3) Adding a catalyst:</em></u>
- Catalyst increases the rate of the reaction without affecting the equilibrium position.
- Catalyst increases the rate via lowering the activation energy of the reaction.
- This can occur via passing the reaction in alternative pathway (changing the mechanism).
- The activation energy is the difference in potential energies between the reactants and transition state (for the forward reaction) and it is the difference in potential energies between the products and transition state (for the reverse reaction).
- in the presence of a catalyst, the activation energy is lowered by lowering the energy of the transition state, which is the rate-determining step, catalysts reduce the required energy of activation to allow a reaction to proceed and, in the case of a reversible reaction, reach equilibrium more rapidly.
- with adding a catalyst, both the forward and reverse reaction rates will speed up equally, which allowing the system to reach equilibrium faster.
- <em>so, the right match is: B) No effect.</em>
Answer:
A
Explanation:
A is the answer because it is explaining how wolves are ancestors of dogs
Glittering in the light
Opaque, not transparent
Light to the hold
D-block element
Since you did not give the reactions, i cannot give the answers.
In organic and inorganic chemistry, nucleophilic substitution is a fundamental class of reactions in which an electron rich nucleophile selectively bonds with or attacks the positive or partially positive (+ve)charge of an atom or a group of atoms to replace a leaving group; the positive or partially positive atom is referred to as an electrophile. The whole molecular entity of which the electrophile and the leaving group are part is usually called the substrate.
The most general form for the reaction may be given as the following:
<span>Nuc: + R-LG → R-Nuc + LG<span>:</span></span>
Answer:
190.2 grams
Explanation:
each arrow points to the amount it weighs, just add it all up
