Answer:
removing the Cl₂ as it is formed
.
adding more ICl(s)
.
removing some of the I₂(s).
Explanation:
<em>Le Châtelier's principle </em><em>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>1) Decreasing the volume of the container:</u>
- Decreasing the volume of the container will increase the pressure.
- 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 no moles of gases and the products side (right) has 1.0 mole of gases.
- So, increasing the pressure will shift the reaction to the side with lower moles of gas (left side) and so the total amount of Cl₂ produced is decreased.
so, decreasing the volume of the container will decrease the total amount of Cl₂ produced.
<u>2) Removing the Cl₂ as it is formed:</u>
- Removing Cl₂ gas will decrease the concentration of the products side, so the reaction will be shifted to the right side to suppress the decrease in the concentration of Cl₂ gas by removing and so the total amount of Cl₂ produced is increased.
so, removing the Cl₂ as it is formed will increase the total amount of Cl₂ produced.
<u><em>3) Adding more ICl(s)
:</em></u>
- Adding ICl(s) 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 ICl(s) by addition and so the total amount of Cl₂ produced is increased.
so, adding more ICl(s) will increase the total amount of Cl₂ produced.
<u>2) Removing some of the I₂(s):</u>
- Removing I₂ gas will decrease the concentration of the products side, so the reaction will be shifted to the right side to suppress the decrease in the concentration of Cl₂ gas by removing and so the total amount of Cl₂ produced is increased.
so, removing some of the I₂(s) will increase the total amount of Cl₂ produced.
<em>the following changes will increase the total amount of of Cl2 that can be produced:</em>
- removing the Cl₂ as it is formed
.
- removing some of the I₂(s).
Answer:
pH measures ratio of H+ ions to OH- ions of substances
pOH measures ratio of OH- ions to H+ ions of substances
Explanation:
pH is a scale which measures the ratio of H+ ions to OH- ions to identify how acidic or basic a substance is. This is because acidic substances have high amounts of H+ ions and low amounts of OH- ions, and therefore have a higher ratio of H+ to OH- ions. (And vice versa for bases, low H+ to OH- ratio) On a pH scale, acidic substances have a pH of 0 to 7, water (neutral pH, not acidic nor basic) has a pH of 7, and bases have a pH of 7-14.
pOH is very similar to pH but measures the opposite: the ratio of OH- ions (indicative of a base) to H+ ions (indicative of an acid). Therefore the pH values are reversed on the scale: Basic substances have pOHs below 7, and acidic substances are above 7 on the pOH scale.
Fundamentally, these two scales measure the same thing is the same way, one just measures the ratio one way (H+:OH-), while the other measured them the other way (OH-:H+), resulting in flipped values on the scales:
pH: 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
<---Acidic---> <------Basic------->
pOH: 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
<----Basic----> <-----Acidic------->
Hope this helped!
Answer:
1.45 x 10⁻² g CO₂
Explanation:
To find the mass of carbon dioxide, you need to (1) convert grams CH₄ to moles CH₄ (via molar mass), then (2) convert moles CH₄ to moles CO₂ (via mole-to-mole ratio from reaction coefficients), and then (3) convert moles CO₂ to grams CO₂ (via molar mass). The final answer should have 3 sig figs to reflect the given value (5.30 x 10⁻³ g).
Molar Mass (CH₄): 12.011 g/mol + 4(1.008 g/mol)
Molar Mass (CH₄): 16.043 g/mol
Combustion of Methane:
1 CH₄ + 2 O₂ ---> 2 H₂O + 1 CO₂
Molar Mass (CO₂): 12.011 g/mol + 2(15.998 g/mol)
Molar Mass (CO₂): 44.007 g/mol
5.30 x 10⁻³ g CH₄ 1 mole 1 mole CO₂ 44.007 g
--------------------------- x ---------------- x --------------------- x ----------------- =
16.043 g 1 mole CH₄ 1 mole
= 0.0145 g CO₂
= 1.45 x 10⁻² g CO₂
Answer:
I think it will option B it will retain enough heat
