Consider the following reaction, which is spontaneous at room temperature. C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) Is ΔS positive or negative? what about ΔH ? Explain. Answer in no more than two sentences.
So for a spontaneous reaction ∆G should be negative, so we have ∆G = ∆H -T∆S so from this condition ∆G will be negative when ∆H is negative and ∆S has to be positive ( since it is -T∆S).
Hence ∆H negative and ∆S to be positive.... Answer
Consider the following reaction, which is spontaneous at room temperature. C3H8(g) + 5O2(g) → 3CO2(g) +...
Consider the combustion of propane: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O(l) ΔH = –2221 kJ Assume that all of the heat comes from the combustion of propane. Calculate ΔH in which 5.00 g of propane is burned in excess oxygen at constant pressure.
Consider the following reaction: C3H8+5O2→3CO2+4H2OC3H8+5O2→3CO2+4H2O What is the reducing agent? C3H8C3H8 CC OO O2
The combustion of propane, C3H8, occurs via the reaction C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) C3H8 (g)= -104.7 CO2(g)= −393.5 H2O(g)= −241.8 Calculate the enthalpy for the combustion of 1 mole of propane.
GIVEN INFO LP gas burns according to the following exothermic reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) ΔH∘rxn= −2044kJ What mass of LP gas is necessary to heat 1.4 L of water from room temperature (25.0 C) to boiling (100.0 C)? Assume that during heating, 16% of the heat emitted by the LP gas combustion goes to heat the water. The rest is lost as heat to the surroundings. Express your answer using two significant figures. FINAL ANWSER SHOULD BE IN GRAMS ?
Propane (C3H8)burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate ΔH∘rxnΔ for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/molkJ/mol.) Express the enthalpy in kilojoules to four significant figures.
The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 7.5 mol of O2 with 1.4 mol of C3H8 will produce ________ mol of CO2. Group of answer choices.
Propane (C3H8) burns in oxygen to produce carbon dioxide and water via the following reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate the mass of CO2 that can be produced if the reaction of 49.9 g of propane and sufficient oxygen has a 60.0 % yield.
Consider the following equilibrium reaction: C3H8 (g) + 5O2 (g) -> 3CO2 (g) + 4 H2O (l) delta H = -2220KJ if the amount of H2) is reduced to the system, the CO2 concentration increases. select one: a) Right b) False
The propane fuel (C3H8) used in gas barbecues burns according to the following equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2044kJ PART A: If a pork roast must absorb 2.3×103kJ to fully cook, and if only 10.% of the heat produced by the barbecue is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?
A.) Classify reaction as exothermic or endothermic. Gas burning in a Bunsen burner: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)+2044kJ B.) Give ΔH for reaction above. C.) Classify reaction as exothermic or endothermic. Dehydratation hydroxide: Co(OH)2(s)+16kJ→CoO(s)+H2O(l) D.) Give ΔH for reaction above. E.) Classify reaction as exothermic or endothermic. Formation of aluminum oxide and chromium from aluminum and chromium (III) oxide: 2Al(s)+Cr2O3(s)→Al2O3(s)+2Cr(s)+536kJ F.) Give ΔH for reaction above.