Answer: 3. H2O(l) -> H2O(g)
Explanation: Entropy is a measure of the randomness or disorder a substance. Gasses have the greatest amount of entropy and solids have the least amount of entropy. The entropy of a sample of H2O increases as liquid water evaporates and changes to a gas.
Answer:
477 °C
Explanation:
Step 1: Given data
- Initial pressure (P₁): 1.0 atm
- Initial temperature (T₁): 27 °C
- Final pressure (P₂): 2.5 atm
Step 2: Convert 27 °C to Kelvin
We will use the following expression.
K = °C + 273.15 = 27 + 273.15 = 300 K
Step 3: Calculate the final temperature (T₂)
If we assume constant volume (before the can explodes) and ideal behavior, we can calculate the final temperature using Gay-Lussac's law.
T₁/P₁ = T₂/P₂
T₂ = T₁ × P₂/P₁
T₂ = 300 K × 2.5 atm/1.0 atm = 750 K
In Celsius,
°C = K - 273.15 = 750 - 273.15 = 477 °C
<span>A 18 M solution of an acid that ionizes only slightly in solution would be termed
concentrated and weak. The concentration of the acid is high. The acid which dissociates partially in water is a weak acid.
</span><span>Calculate the [H^+] for the aqueous solution in which [OH^-] is 1 x10^-9. Is this solution acidic, basic or neutral. To determine [H+] use:
1x10^-14 = [OH-][H+]
solve for [H+]
[H+] = 1x10^-14/1x10^-9
= 1x10^-5</span>
Answer:
Heating water until it boils. The water particles would gain thermal energy from the heat source and there would be an increase in the kinetic energy between the water particles. During this stage, the temperature of the water particles remains the same as the thermal energy is used to break the strong bonds of attraction between the water particles so that they can be further apart and transition from the liquid state to the gas state.