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?
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Consider our dear friend, the combustion of methane/natural gas: CH4 (g) + 2 O2 (g) →...
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)
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 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 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.
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 )
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?
Problem 2 CH 25 C Products 150 C Air 100 25 C Cooling water Methane (CH4) is oxidized with air to produce formaldehyde (HCHO) in a continuous reactor via the following reaction: A competing reaction is the combustion of methane to form CO2: In this specific problem, CH4 and O2 enter the reactor at a mole ratio of 1:1. In the reactor, 40% of CH4 is consumed. Of this 40%, 75% reacted via reaction (1) and the other 25% reacted...
A reaction to produce “substitute natural gas” is described by: 4 CO (g) + 8 H2 (g) → 3 CH4 (g) + CO2 (g) + 2 H2O (l) Use the following information, as necessary, to estimate DH for the above reaction. 2 C (graphite) + O2 (g) → 2 CO (g)ΔfH= –221.0 kJ/mol 2 CO (g) + O2 (g) → 2 CO2(g)ΔrH= –566.0 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (l)ΔfH= –571.6 kJ/mol C (graphite) + 2...
Which of the following equations correctly describes the combustion of methane (CH4) gas? a. CH4 + 1/2O2 --> CO2 + H2O b. CH4 + O2 --> CO2 + H2O C. CH4 + O2 --> CO2 + 2 H2O d. CH4 + 2 O2 --> CO2 + 2 H2O e. CH4 + 3 O2 --> 2 CO2 + H2O
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...