Answer:
Since 2H₂ + O₂ ---> 2H₂O
We need 2 moles of hydrogen for each mole of oxygen
So, we need 2(6) = 12 moles of H₂ but since we only have 10 moles,
H₂ is the limiting reagent
So since 2 moles of H₂ gives 2 moles of water,
10 moles of H₂ will give rise to 10 moles of Water with 1 mole of remaining oxygen
Answer:
The final temperature of the water mixture is 47.85°C
Explanation :
Given,
For Warm Water
mass = 10grams
Temperature = 105°C
For Cold Water
mass = 25grams
Temperature = 25°C
When a sample of warm water is mixed with a sample of cool water,
The energy amount going out of the warm water is equal to the energy amount going into the cool water. This means:
<h3>Qlost = Qgain</h3>
However,
Q = (mass) (ΔT) (Cp)
Cp = Specific heat of water = 4.184 J/Kg°C
So,
(mass) (ΔT) (Cp) = (mass) (ΔT) (Cp)
We start by calling the final, ending temperature 'x.' Keep in mind that BOTH water samples will wind up at the temperature we are calling 'x.' Also, make sure you understand that the 'x' we are using is FINAL temperature. This is what we are solving for.
The warmer water goes down from to 105°C to x, so this means its Δt equals 105°C − x. The colder water goes up in temperature, so its Δt equals x − 25℃
Substituting the values,
(10)( 105°C − x)(4.184) = (25)(x − 25℃)(4.184)
Solving for x, we get
x = 47.85°C
Therefore, The final temperature of the water mixture is 47.85°C.
Answer:
A. 0.0005u
Explanation:
The mass of an electron in amu = 9.1*10-311.66*10-27=0.0005u.
Answer:
100%
Explanation:
My teacher just asked this question.
