A 10-gram aluminum cube absorbs 677 joules when its temperature is increased from 50°c to 125°c. what is the specific heat of al
1 answer:
What is the specific heat of aluminum?
The specific heat of aluminum is 0.90J/g°C.
Given:
Heat absorbs = 677 J
Mass of the substance = 10 g
Initial temperature = 50°C
Final temperature = 125°C
Formula used:
Q = m x c x ΔT
which can also be written as,
Q = m x c x ( -
)
where,
Q = heat absorbs
m = mass of a substance
c = heat capacity of aluminum
= Final temperature
= Initial temperature
Now, put all the values in the formula given above to get the specific heat of aluminum,
677g = (10g) x c x (125 - 50)°C
c = 0.9026 J/g°C
c = 0.90 J/g°C
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Explanation:
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Ethanol (CH₃CH₂OH)
Carbon dioxide (CO₂) = 2.25 l
Pressure = 1 atm
T = 295°K
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C₆H₁₂O₆ ⇒ 2C₂H₅OH(l) +2CO₂(g)
- Calculate the number of moles
PV = nRT
Solve for n
Substitution
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n = 0.092
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1 mol of glucose --------------- 2 moles of carbon dioxide
x --------------- 0.092 moles
x = (0.092 x 1) / 2
x = 0.046 moles of glucose
Molecular weight of glucose = 180 g
180 g of glucose --------------- 1 mol
x g ---------------0.046 moles
x = (0.046 x 180) / 1
x = 8.28 g of glucose
Answer:
Explanation:
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In this case, according to the given chemical reaction for this problem about stoichiometry:
Whereas there is a 3:2 mole ratio of oxygen (molar mass = 32.0 g/mol) to iron (III) oxide (molar mass = 159.69 g/mol) and therefore, the correct stoichiometric setup is:
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