Answer:
The final volume of the cylinder is 1.67 L
Explanation:
Step 1: Data given
Initial volume = 0.250 L
external pressure = 2.00 atm
Expansion does 288 J of work on the surroundings
Step 2: Definition of reversible work:
Wrev = -P(V2-V1) = -288 J
The gas did work, so V2>V1 (volume expands) and the work has a negative sign.(Wrev<0)
V2 = (-Wrev/P) + V1
⇒ with Wrev = reverse work (in J)
⇒ with P = the external pressure (in atm)
⇒ with V1 = the initial volume
We can see that your pressure is in atm and energy in J
To convert from J to L * atm we should use a convenient conversion unit using the universal gas constants :
R
=
8.314472 J/mol
*K and R= 0.08206 L*atm/K*mol
V2 =- (-288 J * (0.08206 L*atm/K*mol /8.314 J/mol
*K))/2.00 atm + 0.250L
V2 = 1.67 L
The final volume of the cylinder is 1.67 L
The question is incomplete, here is the complete question:
Calculate the mole fraction of the ionic species KCl in the solution A solution was prepared by dissolving 43.0 g of KCl in 225 g of water.
<u>Answer:</u> The mole fraction of KCl in the solution is 0.044
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
Given mass of water = 225 g
Molar mass of water = 18 g/mol
Putting values in equation 1, we get:
Given mass of KCl = 43 g
Molar mass of KCl = 74.55 g/mol
Putting values in equation 1, we get:
Mole fraction of a substance is given by:
Moles of KCl = 0.577 moles
Total moles = [0.577 + 12.5] = 13.077 moles
Putting values in above equation, we get:
Hence, the mole fraction of KCl in the solution is 0.044
Answer:
The 2.8 hrs one i think???
hope this helps
Explanation:
Answer:
The 264.61 g food will contain 2150 calories.
Explanation:
Given data:
mass of food = 16 g
calories in 16 g of food = 130 cal
grams of 2150 calories = ?
Solution:
we will solve this problem by cross multiplying.
16 g/ 130 cal = x/2150 cal
x = (16 g/130 cal) × 2150 cal
x = 0.123 g × 2150
x= 264.61 g
so the 264.61 g food will contain 2150 calories.
Answer: The true statements are following:
- Energy of the universe is constant; the entropy of the universe increases.
- If a process increases the randomness of the particles of a system, the entropy of the system increases.
- All spontaneous processes release heat.
- Both and must equal zero at equilibrium.
Explanation:
Spontaneous reactions are defined as the reaction which occur on its own and they do not require any external force to start.
- All spontaneous reactions show a positive value for change in entropy. Each spontaneous reaction requires different amount of time.
Hence, the statement all spontaneous reactions occur quickly, is false.
- Entropy of the Universe always increases and energy always changes from one form to another. Hence, the statement energy of the universe is constant; the entropy of the universe increases, is true.
- As entropy is the degree of randomness. So, with increases the randomness of the particles of a system there will also be increase in randomness.
Therefore, the statement if a process increases the randomness of the particles of a system, the entropy of the system increases, is true.
- Some processes are non-spontaneous in nature. Hence, the statement all systems become more disordered spontaneously, is false.
- Since, randomness between the molecules increases so, heat is eventually released in all spontaneous processes. Therefore, the statement all spontaneous processes release heat, is true.
- For a reversible process, entropy change of the Universe is equal to 0. Therefore,
Hence, the statement both and must equal zero at equilibrium, is true.