how do i find the molar heat of a substance A sample of ethanol (C2H6O) has a mass of 0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.45 J/g•°C. please go step by step

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how do i find the molar heat of a substance A sample of ethanol (C2H6O) has a mass of 0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.45 J/g•°C. please go step by step

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You have to do this in two steps, first find the heat produced by the sample, using the information given and this equation: \(\sf q=m_{water}*C_p*\Delta T\) Next, we'll convert the mass of the sample of ethanol to moles (moles is denoted by \(\sf n\) in the equation below). We will use that and and the heat found in the first step. \(\sf q=\Delta H^o_{comb}* n\rightarrow \Delta H^o_{comb}=\dfrac{q}{n}\)
wait what is the delta H?
This is what I think, The specific Heat formula \[\Delta{Q}=mc \Delta{T}\] where c= Specific Heat Capacity \[\Delta{Q}=\] Heat required for the temperature change or Thermal energy change \[\Delta{T}=\] Change in Temperature m= Mass of the object Substituting numbers, you will get q. and after that put it in \[q = n ΔH _{trans}\] where "trans" will be one of the following: fusion, freezing, evaporation, condensation, sublimation, or deposition

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Substances not changing phase: q = m Cs ΔT (per gram) q = n Cm ΔT (per mol) Substances that are changing phase (transition): q = m ΔHtrans (per gram) q = n ΔHtrans (per mol)
\[\Delta{H}=Enthalpy Change\]
ok thanks you helped alot

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