Answer:
The exposed metal rusts is an example of a chemical change because rust is an example of a chemical change in objects for example bicycles, scooters, etc.
Answer:
only one atom of that element
Explanation:
Example:
H2 O has two hydrogenatoms and ONE Oxygen atom
Answer:
1) Increasing the pressure A) Shift to the left
2) Removing hydrogen gas B) Shift to the right
3) Adding a catalyst C) 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) Decreasing 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, decreasing the pressure will shift the reaction to the side with more moles of gas (left side).
<u><em>so, the right match is: A) Shift to the left.</em></u>
<em><u>2) Adding hydrogen gas:</u></em>
- Adding hydrogen gas will increase the concentration of the reactants side, so the reaction will be shifted to the right side to suppress the increase in the concentration of hydrogen gas by addition.
<u><em>so, the right match is: B) Shift to the right.</em></u>
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<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.
<u><em>so, the right match is: B) No effect.</em></u>
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Explanation:
it's probably gonna be the secondary consumer, energy is lost/reduced as it goes up the food chain
(2) A corn field is an ecosystem, in it, you'll find the interaction of both animals, insects, microorganisms and plants in it
2C6H14 + 19O2 ===> 12CO2 + 14H2O ... balanced equation
moled hexane present = 2.6 g x 1 mole/130 g = 0.02 moles
moles O2 present = 5.29 g x 1 mole/32 g = 0.165 moles
Which reactant is limiting? Hexane = 0.02/2 = 0.01; O2 = 0.165/19 = 0.0087
Thus O2 is limiting...
moles of H2O that can be produced =0.165 moles O2 x 14 H2O/19 CO2 = 0.122 moles H2O
Mass H2O = 0.122 moles x 18 gm/mole = 2.20 g (to 3 sig. figs.)
