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carminelouse619Lv1

11 Dec 2019

burning of 15.5 g of propane: c3h8(g)+5o2(g)→3co2(g)+4h2o(l) δh∘=−2220 kj

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Miguel MatienzoLv10

17 Mar 2021

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Calculate the enthalpy change when 11.0 g of carbon dioxide forms from the combustion of propane.

C₃H₈(g) + 5O₂(g) â 3CO₂(g) + 2H₂O(l)

ÎH = -2220 kJ

Thermochemical equivalencies:

1 mol propane = 5 mol oxygen = 3 mol carbon dioxide = 4 mol water = 2220 kJ

Calculate the free energy change for the following reaction at 25 ∘C.

C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)

ΔH∘rxn= -2217 kJ

ΔS∘rxn= 101.1 J/K.

chocolatefrog316

Propane, C3H8, is used in many instances to produce heat by burning: C3H8(g) + 5O2(g) â 3CO2(g) + 4H2O(g) The standard enthalpy of reaction, ÎHrxn, is â2,044 kJ. ÎHrxn is a symbol or the heat of reaction. 1. How many grams of oxygen would be needed to produce 396.0 kJ of heat?

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burning of 15.5 g of propane: c3h8(g)+5o2(g)→3co2(g)+4h2o(l) δh∘=−2220 kj

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