Answer:
And we have to calculate the number of moles of sucrose present in a lb mass of sucrose: Moles of sucrose=454⋅g342.30⋅g⋅mol−1=1.33⋅mol .
Explanation:
<u>Brainliest</u><u> </u><u>Answer </u><u>Pls</u>
Particles in a gas have more energy than particles in a liquid. Because in gaseous state particles are free to move around due to which kinetic energy of molecule or gas increases and hence overall energy increases
Answer:
N = 5.8 × 10²⁴ molecules
Explanation:
Step 1: Given and required data
- Moles of C₂H₄ (n): 9.6 mol
- Avogadro's number (NA): 6.02 × 10²³ molecules/mol
Step 2: Calculate the number of molecules (N) in 9.6 moles of C₂H₄
To convert moles to molecules we need Avogadro's number: there are 6.02 × 10²³ molecules of C₂H₄ per mole of C₂H₄
N = n × NA
N = 9.6 mol × 6.02 × 10²³ molecules/mol
N = 5.8 × 10²⁴ molecules
Answer:
16974J of energy are required
Explanation:
The energy required is:
* The energy to heat solid water from -15°C to 0°C using:
q = m*S*ΔT
* The energy to convert the solid water to liquid water:
q = dH*m
* The energy required to increase the temperature of liquid water from 0°C to 75°C
q = m*S*ΔT
The first energy is:
q = m*S*ΔT
<em>m = Mass water = 25g</em>
<em>S is specific heat of ice = 2.03J/g°C</em>
<em>ΔT is change in temperature = 0°C - (-15°C) = 15°C</em>
q = 25g*2.03J/g°C*15°C
q = 761.3J
The second energy is:
q = dH*m
<em>m = Mass water = 25g</em>
<em>dH is heat of fusion of water = 80cal/g</em>
q = 80cal/g*25g
q = 2000cal * (4.184J/1cal) = 8368J
The third energy is:
q = m*S*ΔT
<em>m = Mass water = 25g</em>
<em>S is specific heat of water= 4.184J/g°C</em>
<em>ΔT is change in temperature = 75°C-0°C = 75°C</em>
q = 25g*4.184J/g°C*75°C
q = 7845J
The energy is: 7845J + 8368J + 761J =
16974J of energy are required
