The thermochemical equation of combustion of methane is:
CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l)
ΔΗ =-890.3 kJ
1. Calculate the AH when 5.00 g CH4 react with excess of oxygen.
2. Calculate AH when 2L CH4 at 49 °C and 782 mmHg react with an excess of oxygen
3. Calculate AH when 2L CH4 react with L O2 in a reaction vessel kept at 49 °C and 782 mmHg.
The thermochemical equation of combustion of methane is: CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l)
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?
The thermochemical equation for the combustion of ethanol is: 5. C2H&OH (I)+3 O2 (g) 2 CO2 (g)+3 H2O (g) AH-1360 kJ What is the enthalpy change when 3.50 kg of ethanol react with excess oxygen?
The thermochemical equation for the combustion of ethanol is: C2H5OH (l) + 3 O2 (g) -> 2 CO2 (g) + 3 H2O (g) ΔHrxn = -1360 kJ What is the enthalpy change when 3.50 kg of ethanol react with excess oxygen?
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.
given the following thermochemical equation detailing the combustion of methane (CH4) determine the amount of energy released when 1.563 mol of methane undergoes combustion Given the following thermochemical equation 14. detailing the combustion of methane (CH4) CH g)+ 202(g) CO2(g) + 2H20(g) 1.563 determine the amount of energy released when 1.563 mol of methane undergoes combustion. AH=-802kJ/mol CH a. 1.95 x d. 1250 kJ b. 3,12x 10 kJ e. 2.01 x 10' kJ c. 453 kJ
The following thermochemical equation is for the reaction of methane(g) with oxygen(g) to form carbon dioxide(g) and water(g). CH4(g) + 2O2(g) ---> CO2(g) + 2H2O(g) H = -802 kJ When 6.37 grams of methane(g) react with excess oxygen(g), ___ kJ of energy are _________(evolved or absorbed). Once you get the answer, would it be a negative number or a positive number?
Calculate the standard enthalpy of formation of gaseous methane (CH4) using the following thermochemical information: CO2(g) + 2 H2O(l) CH4(g) + 2 O2(g) H = +890.4 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ
CH4(g)+O2(g)→CO2(g)+H2O(g) Part A. What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H2O, respectively. Part B. What mass of carbon dioxide is produced from the complete combustion of 8.30×10−3 g of methane? Part C. What mass of water is produced from the complete combustion of 8.30×10−3 g of methane? Part D. What mass of oxygen is needed for the complete combustion of 8.30×10−3 g of...
what are the products of the combustion reaction of methane CH4, with oxygen CO2(g) and H2O(g) C(s), and H2O(g) H2CO3(aq) CO2(g) only CO(g) and H2(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?