Answer:
3460 mL
Explanation:
We are given:
T(i) = 351 k T(f) = 289 k
V (i) = v mL V(f) = 285 mL
Using the gas equation:
PV = nRT
Since Pressure (P) , number of moles (n) and R is the universal gas constant
We can say that V/T = k (where k is a constant)
Hence, we can say that:
V(i) / T(i) = V(f) / T(f)
Replacing the values
v / 351 = 285 / 289
v = 3460 mL
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Answer:
The amount of heat required to raise the temperature of the sample from 298 to 385 Kelvin, is 16.6 kJ
Explanation:
<u>Step 1: </u>Given data
A 79.0 g sample of ethanol raises from 298 K to 385 K
The specific heat of ethanol is 2.42J/g°C
<u>Step 2:</u> Calculate the heat transfer
Q = m*Cp*ΔT
with m = the mass of the ethanol sample (in grams)
⇒ mass = 79 grams
with Cp = the specific heat capacity of ethanol (in J/g°C)
⇒ Cp = 2.42 J/g°C
with ΔT = the change of temperature (T2-T1)
⇒ ΔT = 385 K - 298K = 112 °C - 25 °C = 87
Q = 79 grams * 2.42 J/g°C * 87 = 16632.66 j = 16.6 kJ
The amount of heat required to raise the temperature of the sample from 298 to 385 Kelvin, is 16.6 kJ
Hence it has been cut into 4pieces