Clarification on Q20 29:15 Exothermic reactions will always have a negative delta H. This is because they are giving out heat energy. And the reverse is true for endothermic. For endothermic, heat is absorbed so delta H is always positive. I didn’t notice this error, and sorry for the inconvenience!!
hi, @olwynblackston8095 for Q17. This particular question is testing you in the knowledge of equilibrium. You have to know Le Chatlier’s Law. It is that when you change a condition in a reaction, the equilibrium will always oppose it. In simple terms, every action or change you bring forth, the equilibrium will always oppose that change in reaction condition to lower/counteract the change you did. In this case, we want BiClO to be dissolved so the reaction we have to look at is the backward reaction. I.e you have to turn it into BiCl3 (aq). To do this you need to do certain changes so that equilibrium will favor or shift to the backward or left side equation. In this case, you can add acid. Adding acid means you are adding H+ ions. When the concentration of H+ ions increases, the equilibrium counteracts that change by converting BiClO with H+ to produce less BiClO and more BiCl3. The same principal applies to adding NaCl solution. When you add NaCl sol, It is the same as adding Na ions and cl- ions. This means you are increasing the ions conc, so equilibrium counteract this and favors the backward reaction to decrease concentration of Na and Cl by using it up and reacting it with BiClO and forming the aqueous BiCl3. I hope I made it easier for you to understand.
Clarification on Q20 29:15 Exothermic reactions will always have a negative delta H. This is because they are giving out heat energy. And the reverse is true for endothermic. For endothermic, heat is absorbed so delta H is always positive. I didn’t notice this error, and sorry for the inconvenience!!
Hello. In 29:15 the enthalpy change of reaction for exothermic is delta -. because more energy is released than absorbed.
thank you so much for pointing it out for others. yes, it’s a mistake on my part. i said the opposite.
Sorry I'm a bit confused on question 17, can anyone explain it?
hi, @olwynblackston8095 for Q17. This particular question is testing you in the knowledge of equilibrium. You have to know Le Chatlier’s Law. It is that when you change a condition in a reaction, the equilibrium will always oppose it. In simple terms, every action or change you bring forth, the equilibrium will always oppose that change in reaction condition to lower/counteract the change you did.
In this case, we want BiClO to be dissolved so the reaction we have to look at is the backward reaction. I.e you have to turn it into BiCl3 (aq). To do this you need to do certain changes so that equilibrium will favor or shift to the backward or left side equation. In this case, you can add acid. Adding acid means you are adding H+ ions. When the concentration of H+ ions increases, the equilibrium counteracts that change by converting BiClO with H+ to produce less BiClO and more BiCl3. The same principal applies to adding NaCl solution. When you add NaCl sol, It is the same as adding Na ions and cl- ions. This means you are increasing the ions conc, so equilibrium counteract this and favors the backward reaction to decrease concentration of Na and Cl by using it up and reacting it with BiClO and forming the aqueous BiCl3.
I hope I made it easier for you to understand.
thank you
speak louder anime kid, ur calculator sounds more confident than you.
No need to comment that
@@savagex_2008 my bad lol I'm joking