For the combustion of methane(CH4) CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O...

Question

Question

For the combustion of methane(CH4)

CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol

If 250.0 g of CH4 is burned , what is the energy change? ( Answers in scientific notation are entered such as 1.234 e4 )

Answer 1

Answer #1

Number of moles CH4 in 250g = amount of the methane/mw of methane= 250g/16.04 g/mole= 15.586 moles

According to the above balanced equation

1 mole of methane combustion produces 882 kJ of heat

Therefore combustion of 15.586 moles of methane will produce = 15.586 X 882 kJ of heat = 1.375 e4 kJ of heat

Answer 2

Similar Homework Help Questions

CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H =...

CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol From the equation above, What is Δ H for the reaction below in kJ/mol. H2O (g)+ 1/2 CO2 (g) --> O2 (g) + 1/2 CH4 (g)
Use the combustion of methane for the following question: CH4 (g) + O2 (g) → CO2...

Use the combustion of methane for the following question: CH4 (g) + O2 (g) → CO2 (g) + H2O (l) ∆H = -890 kJ/mol A)Is the reaction exothermic or endothermic? B)If I combust 2 mol of methane, how much heat is absorbed or released - use the appropriate sign to indicate in your answer. C) If I combust 12.5 g of methane, how much energy in kJ is absorbed or released? Use the appropriate sign in your answer.
The combustion of methane (natural gas) is given by the equation: CH4 (g) + 2 O2...

The combustion of methane (natural gas) is given by the equation: CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) ΔH = -890 kJ How much heat (in kJ) is released by the reaction of 48.5 grams of O2 with excess CH4? Remember that if heat is given off, is negative, and should be entered as such)

For the combustion reaction of methane, AHºf is zero for CH4 (g) + O2 (g) →...

For the combustion reaction of methane, AHºf is zero for CH4 (g) + O2 (g) → 2H2O(g) + CO2 (g) A) 02 (g) B) CH4 (g) CO2 (g) D) H20 (g) E) Both O2 (g) and CH4 (g) 8 Given the following reactions N2 (g) + 202 (g) - 2NO2 (g) AH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) AH = -114.2 kJ the enthalpy of the reaction of the nitrogen to produce nitric oxide N2...
4 For the combustion reaction of methane, AHºf is zero for CH4 (g) + O2 (g)...

4 For the combustion reaction of methane, AHºf is zero for CH4 (g) + O2 (g) → 2H2O(g) + CO2 (g) A) 02 (g) B) CH4 (g) C CO2 (g) B) H20 (g) E) Both O2 (g) and CH4 (g)
Consider the combustion of methane (shown below), CH4(g) + 2 O2(g) --> CO2(g) + 2 H2O(g)...

Consider the combustion of methane (shown below), CH4(g) + 2 O2(g) --> CO2(g) + 2 H2O(g) The rate of change in the concentration of CH4 is –0.045 M/s. What is the rate of formation of H2O?

Consider our dear friend, the combustion of methane/natural gas: CH4 (g) + 2 O2 (g) →...

Consider our dear friend, the combustion of methane/natural gas: CH4 (g) + 2 O2 (g) → 2 CO2 (g) + H2O (l) ΔHreaction = -802.3 kJ/mol If 1.50 mol O2 are consumed, how much heat is produced by this reaction?
The experimentally determined heat of combustion of methane is 50.1 kJ/g. Calculate the heat of combustion...

The experimentally determined heat of combustion of methane is 50.1 kJ/g. Calculate the heat of combustion of methane in kJ/mol. Molar mass of methane CH4 = 16 g/mol CH4(g) + 2 O2(g) → CO2 (g) + 2 H2O(l)
Consider the combustion of methane: CH4 (g) + 2 02 (g) → CO2 (g) + 2...

Consider the combustion of methane: CH4 (g) + 2 02 (g) → CO2 (g) + 2 H2O (g) If 5.00 g of CH4 burns in the presence of 10.0 g O2, determine the limiting reactant and how many grams of CO2 are produced.

Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 ...

PART ONE: PART TWO: PART THREE: PART FOUR: Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 and gaseous water (H20). Suppose 13. g of methane is mixed with 13.8 g of oxygen. Calculate the minimum mass of methane that could be left over by the chemical reaction. Round your answer to 2 significant digits A 1.32-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.85 °C...