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.
A.) Classify reaction as exothermic or endothermic. Gas burning in a Bunsen burner: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)+2044kJ B.) Give...
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 ?
The propane fuel (C3H8) used in gas barbeques burns according to this thermochemical equation. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2044kJ If a pork roast must absorb 1.7×103 kJ to fully cook, and if only 15 % of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?
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?
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.
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.
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.
Please help? Calculate deltaHr for the reaction: C3H8(g) + 5O2(g)----->3CO2(g) + 4H2O(l) Given: 3C(s) + 4H2(g)----->C3H8(g) deltaH -24.8 kcal H2(g) + 1/2 O2(g)----->H2O(l) deltaH -68.3kcal C(s) + O2(g)-------> CO2(g) deltaH -94.0 kcal
Reaction 1: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g), ΔH1=−2043 kJ Reaction 2: 4C3H8(g)+20O2(g)→12CO2(g)+16H2O(g), ΔH2=? Express your answer to four significant figures and include the appropriate units.
1. The dimensions of the SI unit of energy, the Joule (J), are A. K B. kg m s C. kg m2 s-2 D. kg m-1 s-2 E. kg m2 s-1 2. Natural gas, or methane, is an important fuel. Combustion of one mole of methane releases 802.3 kilojoules of energy. How much energy does that represent in kilocalories? A. 3.36×103 kcal B. 3.357 kcal C. 191.8 kcal D. 0.192 kcal E. 1.918×105 kcal 3. What is the change in...