Answer:
100 kPa
Explanation:
This can be solved with one of the gases law. This law establishes that the pressure of the gas is directly proportional to its temperature: If we increase the temperature, the pressure will increase.
In this case, we decrease the temperature, so its pressure will be lower.
P₁ / T₁ = P₂ / T₂
We convert T° to Absolutes Values
27°C + 273 = 300 K
-173°C + 273 = 100 K
300 kPa / 300 K = P₂ / 100 K
(300 kPa / 300 K) . 100K = P₂
P₂ = 100 kPa
This is the Charles Gay Lussac's law.
2 electrons on the first ring, 8 on the second, and 3 on the third ring
No math is needed to explain this. All that you need to know is that the can (4°C) is in your hand (37°C).
Entropy will always move toward being balanced. Never will you find a lake in which half of it is 1°C and the other half is 70°C; it will be equal throughout.
Remember that "cold" doesn't exist. What we describe to be cold is actually a lack of heat.
So, by applying the two ideas above, it can be concluded that:
Since your hand is warmer than the can, the heat from your hand will be transferred to the can in order to reach an equal temperature.
<span>Moles HClO4 = 0.02500 L x 0.723 M=0.0181
moles KOH = 0.0100 L x 0.273 M= 0.00273
total volume = 25.00 + 10.0 = 35.0 mL = 0.0350 L
moles H+ in excess = 0.0181 - 0.00273 =0.0154
[H+]= 0.0154 mol/ 0.0350 L=0.440 M</span>
Answer:
Answer 'A' is correct
Explanation:
For any reaction to occur, 4 events must occur simultaneously. These are...
1. reacting compounds must be at concentrations that allow them to find on another. Such is concentration dependent and is referred to as Kinetic Feasibility.
2. reacting compounds must collide in very specific orientations for bonding to occur. The reacting compounds have unique molecular geometries such that bonding only occurs if the compounds collide in a required orientation.
3. The reacting compounds must have a natural tendency to react and form chemical bonds.
4. The reacting system must be at sufficient temperature (which delivers sufficient energy (ΔEₐ) such that events 1, 2 and 3 have the highest probability of occurring simultaneously. This occurs at the activation energy point (k = A·e^(-ΔEₐ/RΔT) => lnΔk = lnA - ΔEₐ/RΔT) => The Arrhenius Equation of Kinetic Reactivity.