What mass of natural gas (CH4) must you burn to emit 259 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ Express the mass in grams to three significant figures.
What mass of natural gas (CH4) must you burn to emit 259 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ Expres...
What mass of natural gas (CH4) must you burn to emit 258 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ
1. What mass of natural gas (CH4) must you burn to emit 260 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH∘rxn=−802.3kJ 2.Consider the following thermochemical equation for the combustion of acetone, C3H6OC3H6O, the main ingredient in nail polish remover: C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g)ΔH∘rxn=−1790kJ If a bottle of nail polish remover contains 173 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 g/mL 3.Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When...
Part A What mass of natural gas (CH) must you burn to emit 268 kJ of heat? CH4 (g) + 202 (g) + CO2(g) + 2H2O(g) AH = -802.3 kJ Express the mass in grams to three significant figures. O AL M O O ? Submit Request Answer
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) CH4(g) -201 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
What mass of natural gas CH4 must you burn to emit 270 kJ of heat?
The equation for the combustion of CH4 (the main component of natural gas) is shown below. How much heat is produced by the complete combustion of 289 g of CH4? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ
Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔHorxn = -802.3 kJ You may want to reference (Page 269) Section 6.6 while completing this problem.What minimum mass of CH4 is required to heat 85.0 g of water by 23.0 ∘C? (Assume 100% heating efficiency.) (For water,Cs= 4.18 J/g∘C).
4) What mass of natural gas (CH4) must burn so that the heat released by the reaction CH4(g)2 O2(g) CO2(g)+2 H20(g) is 267 kJ. The molar mass of CH4 is 16.0 g mol. The standard enthalpies of formation of some of the substances in the reaction are: AH (CH (g))-74.81 kJ mol AH (CO2(g)-393.509 kJ mol AHP(H20(g)-241.818 kJ mol a) 0.223 g b) 3.57 g c) 0.280 g d 0.623 g e) 1195 g f) 467 g
PART A. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Express your answer using four significant figures. PART B. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Express your answer using three significant figures. PART C. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C(s)+O2(g)→CO2(g) Express your answer using four significant figures. PART D. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction:...
a) Determine the mass of CO2 produced by burning enough of methane to produce 1.50×102kJ of heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ b) Determine the mass of CO2 produced by burning enough of propane to produce 1.50×102kJ of heat. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2217kJ c) Determine the mass of CO2 produced by burning enough of octane to produce 1.50×102kJ of heat. C8H18(l)+25/2O2(g)→8CO2(g)+9H2O(g)ΔH∘rxn=−5074.1kJ d) Which fuel contributes least to global warming per of heat produced? methane propane octane