Answer:
17 kJ
Explanation:
Calculation for the Calculate the energy required to heat 0.60kg of ethanol from 2.2°C to 13.7°C.
Using this formula
q = mC∆T
Where,
q represent Energy
m represent Mass of substance=0.60kg=600g
C represent Specific heat capacity=2.44J·g−1K−1.
∆T represent change in Temperature=2.2°C to 13.7°C.
Let plug in the formula
q=(0.60 kg x 1000 g/kg)(2.44 J/gº)(13.7°C-2.2°C)
q = (600g)(2.44 J/gº)(11.5º)
q=16.836 kJ
q= 17 kJ (Approximately)
Therefore the energy required to heat 0.60kg of ethanol from 2.2°C to 13.7°C will be 17 kJ
I'm not 100% sure but I'm leaning towards D. :)
It's D because I know bcz I'm smart 8 times 8 is 60-nart
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Answer:
1.8 x 10^24
One mole of helium has 6.02 x 10^23 atoms, thise number is also called Avogadro's number or constant.
If we need number of atoms for 3 moles so simply, multiply 3 by 6.02 x 10^23
so,
Number of atoms for 3 moles = 3 x ()
Number of atoms will be = 1.806x10^24
