Answer:
Explanation:
Here, we want to calculate the final volume
We use the general gas equation here:
P1 is the initial pressure which is 0.850 atm
V1 is the initial volume which is 4.25 L
T1 is the initial temperature which is (23 + 273.15 = 296.15 K)
P2 is the final pressure which is 1.50 atm
V2 is the final volume which is unknown
T2 is the final temperature (11.5 + 273.15 = 284.65 K)
Substituting the values, we have:
If there was more water area and less land more animals would adapt to the water life than land. Like for example more evolving fins or even amphibians
just staying in water and no longer needing legs or the things they use for living on the land.
1. 100 C
2. Point B to C is the ices heat capacity
3. During the points D to E the bonds of the water molecules build up enough kinetic energy to break their intermolecular bonds (not intra), which can lead to gas.
4. Between points D and E the energy is being released the energy required is equivalent along the line.
5. Between point E and D the water is converting to water (condensation)
6. Energy is being released 2260 j/g
7. Yes, but only under extreme volumetric pressures
8. D and E or B and C
9. Freezing (the water is also becoming less dense)
10. Melting or if water already, absorbtion of energy
11. released.
Answer:
To increase the yield of H₂ we would use a low temperature.
For an exothermic reaction such as this, decreasing temperature increases the value of K and the amount of products at equilibrium. Low temperature increases the value of K and the amount of products at equilibrium.
Explanation:
Let´s consider the following reaction:
CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)
When a system at equilibrium is disturbed, the response of the system is explained by Le Chatelier's Principle: <em>If a system at equilibrium suffers a perturbation (in temperature, pressure, concentration), the system will shift its equilibrium position to counteract such perturbation</em>.
In this case, we have an exothermic reaction (ΔH° < 0). We can imagine heat as one of the products. If we decrease the temperature, the system will try to raise it favoring the forward reaction to release heat and, at the same time, increasing the yield of H₂. By having more products, the value of the equilibrium constant K increases.
I believe the balanced chemical equation is:
C6H12O6 (aq) + 6O2(g)
------> 6CO2(g) + 6H2O(l)
First calculate the
moles of CO2 produced:
moles CO2 = 25.5 g
C6H12O6 * (1 mol C6H12O6 / 180.15 g) * (6 mol CO2 / 1 mol C6H12O6)
moles CO2 = 0.8493 mol
Using PV = nRT from
the ideal gas law:
<span>V = nRT / P</span>
V = 0.8493 mol *
0.08205746 L atm / mol K * (37 + 273.15 K) / 0.970 atm
<span>V = 22.28 L</span>
