Answer:
a) and d) are false.
Explanation:
a) The second law of thermodynamics states that t<u>he entropy of the universe increases in a spon
taneous process and remains unchanged in an equilibrium process.</u>
For a spontaneous process:
ΔSuniv = ΔSsys + ΔSsurr > 0
For a spontaneous process, the second law says that ΔSuniv must be greater than zero, but it does not place a restriction on either ΔSsys or ΔSsurr. Thus, it is possible for either ΔSsys or ΔSsurr to be negative, as long as the sum of these two quantities is greater than zero.
d) <u>A reaction that does occur under the given set of conditions is called a</u> spontaneous reaction. We observe spontaneous physical and chemical processes every day, including many of the following examples:
• A waterfall runs downhill, but never up, spontaneously.
• A lump of sugar spontaneously dissolves in a cup of coffee, but dissolved sugar does not spontaneously reappear in its original form.
• Heat flows from a hotter object to a colder one, but the reverse never happens spontaneously.
Answer:
letter b
Explanation:
I dunno if I'm right cuz I'm just a grade five sorry if this can't help
Answer: 3.41 mL
Explanation: Solution:
Use Combine gas law to solve this problem.
P1V1 / T1 = P2V2 / T2
First convert temperature to K
T1 = 47 °C + 273 = 320 K
T2= 107°C + 273 = 380 K
Derive to find V2:
V2 = P1 V1 T2 / T1 P2
Substitute the values:
V2= 1.03 atm x 2.20 mL x 380 K /
320 K x 0.789 atm
= 3.41 mL
Cancel out the units of atm and K so the remaining unit is in mL.
Answer:
C) Heat will transfer from the water to the air
Explanation:
