Given the following data:
2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ΔH = -2600 kJ
C2H2(g) + 2H2(g) → C2H6(g) ΔH = -312 kJ
2H2(g) + O2(g) → 2H2O(l) ΔH = -572 kJ
Find the ΔH of the following reaction: 4CO2(g) + 6H2O(l) → 2C2H6(g) + 7O2(g)
Given the following data: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ΔH = -2600 kJ C2H2(g)...
Use the set of three reactions shown below to answer the questions that follow. 2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ 2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ If 27.9 g of NO g is reacted with excess oxygen, how much heat energy is produced? What mass of liquid water will be consumed during the production of 33900 J of energy assuming that there is...
Find ∆H◦ of the reaction 2C2H2(g) + 5O2(g) = 4CO2(g) + 2H2O(g), as it is written, given the following: 2C(s) + H2(g) = C2H2(g), ∆H◦ = +227.4 kJ, 2H2(g) + O2(g) = 2H2O(g), ∆H◦ = −483.6 kJ, C(s) + O2(g) = CO2(g), ∆H◦ = −393.5 kJ.
8. Find ∆H◦ of the reaction 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(g), as it is written, given the following: 2C(s) + 3H2(g) = C2H6(g), ∆H◦ = −84.68 kJ, 2H2(g) + O2(g) = 2H2O(g), ∆H◦ = −483.6 kJ, C(s) + O2(g) = CO2(g), ∆H◦ = −393.5 kJ. (A) −3194 kJ (B) −3109 kJ (C) −2940 kJ (D) −2855 kJ (E) −1428 kJ
all 3. Calculate the heat released (kJ) in the reaction of 1.35L of acetylene (C2H2) and 0.235L of hydrogen gas at STP to form ethane gas as determined by the following equation: C2H2(g) + 2H2() → C2H6(g) Given: 2C2H2(g) +502(g) + 4CO2(g) + 2H20(g) 2C2H.(g) + 702(g) → 4CO2(g) + 6H20(g) 2H2(g) + O2(g) → 2H2O(g) AH = -2320 kJ/mol AH = -3040 kJ/mol AH = -572 kJ/mol
2C2H2+5O2=4CO2+2H2O If one starts with 4 moles of O2, how many moles of C2H2 will react with it? How many moles of CO2 will be produced? How many moles of H2O will be produced? Starting with 15 moles of C2H2, how many moles of O2 are required to react with it? How many moles of CO2 will be produced? How many moles of H2O will be produced?
Consider the exothermic reaction 2C2H6(g)+7O2(g)→4CO2(g)+6H2O(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) C2H6(g) -84.7 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
The combustion of acetylene C2H2, takes place according to the equation: 2C2H2 + 5O2 ---> 4CO2 + 2H2O; delta H is -5198 kJ In an experiment, 0.338 g C2H2 is combusted in a bomb calorimeter. If the heat capacity of the calorimeter is 729 J/K and it contains 1/150 kg of water, what is the temperature increase of the bomb calorimeter? The spedicif heat capacity of water is 4/184 J/g.K
2C2H2+5O2=4CO2+2H2O Starting with 130g of C2H2, how many grams of O2 are required? How many grams of CO2 are produced? How many grams of H2O are produced? If one produced 360g of CO2, how many grams of C2H2 did one start with? How many grams of O2 are required? How many grams of water were produced? Please show work!
2C2H2+5O2=4CO2+2H2O If one starts with 4 moles of O2, how many moles of C2H2 will react with it? How many moles of CO2 will be produced? How many moles of H2O will be produced? Starting with 15 moles of C2H2, how many moles of O2 are required to react with it? How many moles of CO2 will be produced? How many moles of H2O will be produced? Starting with 130g of C2H2, how many grams of O2 are required? How...
2C2H6 (g) + 7O2 (g) → 4CO2(g) + 6H2O (g) ΔH = -1560 kJ How much heat (in kJ) is released if 17.9 g of ethane ( 30.07 g/mol) undergoes combustion? (Give your answer as a positive number, since you cannot release negative energy.)