Answer:
I. Increasing pressure will allow more frequent successful collision between particles due to the particles being closer together.
II. Rate of reaction increases due to more products being made; as increased pressure favours the exothermic side of the equilibrium.
III. Increasing temperature provides particles lots of (Kinetic) energy, for more frequent successful collision due to the particles moving at a faster rate than before. However, favouring the endothermic side of the equilibrium due to lots of energy required to break and form new bonds.
IV. Rate of reaction increases due to increase temperature favouring both directions of the equilibrium - causing products to form faster.
Hope this helps!
Answer:
The answers are as given in the attachment
Explanation:
The application of the de brogile equation was used and appropriate substitution were made as shown in the attachment
-III I
NH₄⁺
V -II
N₂O₅
I V -II
NaNO₃
-----------------------
-3 +5 +5
Yes you can use that 1 equation.. P1V1/(n1T1) = P2V2/(n2T2) for ALL of your two state ideal gas law type problems. Use it in place of boyles, charles, avogadros, combined, etc laws...just like I showed you above
<span>(1).. write down P1V1/(n1T1) = P2V2/(n2T2) </span>
<span>(2).. rearrange for your desired unknown </span>
<span>(3).. determine what is constant and what varies.. cancel the constants </span>
<span>(4).. plug and chug.. don't forget Temperature must be on an absolute scale.. R or K.. never °F nor °C </span>
Two animals that are omnivores are:
Bears and Badgers
Bears eat clover and other plants, and they eat salmon and other animals.
Badgers eat plants such as different fruits like pears and plums, and Badgers eat earthworms, insects, amphibians (such as frogs) reptiles and birds.
