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.
thank you vmuch....
Use the combustion of methane for the following question: CH4 (g) + O2 (g) → CO2...
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)
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?
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 )
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 (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 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.
Thermochemistry Consider the combustion of propane: AH (k/mol) -105 substance CaHs (g) CO2 (g) O2 (g) H2O (g) 3 CO2 (g) + 4 H20 (g) CaHe (g) + 5 02 (g) -394 0 Use the heats of formation in the table to calculate AHatons -242 Is this reaction exothermic or endothermic? Explain your choice. The surroundings would become (circle one) cooler warmer Energy is (circle one) released from absorbed by the reaction.
A chemist measures the energy change AH during the following reaction: CH4(9)+202(9) + CO2(9)+2H2O(1) AH= -882. kJ Use the information to answer the following questions. This reaction is... ОО endothermic. exothermic. Yes, absorbed. Yes, released. Suppose 33.5 g of CH4 react. X 5 ? Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer...
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...
Given the following thermochemical equation for the combustion of methane gas: CH4 (9) + 2O2 (g) → CO2 (g) + 2H20 (1) AH = -890 kJ How many grams of methane are required to produce 132 kJ of energy?