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Determine the heat of combustion of acetylene (C2H2).
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If heat of combustion of acetylene C2H2 is -1301.1 kJ/mol then :
a) Write balanced thermochemical equation of acetylene
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I think it's so : a) 2C2H2 + 5O2 => 4CO2 + 2H2O + 1301.1kJ b) 0.25mol * 1301.1 kJ = 325.27 kJ energy
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Determine the heat of combustion of acetylene (C2H2).
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To determine the heat of combustion of acetylene (C2H2), we need to use the balanced chemical
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Determine the heat of combustion of acetylene (C2H2).
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C2H2 +5/2 O2 ==> 2CO2 + H2O I would look up the deltaHf for CO2 and for H2O as well as C2H2. Then
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Determine the heat of combustion of acetylene (C2H2).
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To determine the heat of combustion of acetylene (C2H2), you can use the principles of Hess's Law
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To determine the heat of combustion of acetylene (C2H2), you'll need to follow a few steps: 1. Write
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Acetylene(C2H2) torches are used in welding.
How much heat (in kJ) evolves when 2.0L of C2H2 (d=1.0967kg/m3) is mixed with a
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Convert 2.0 L acetylene to grams using density. q = heat evolved = 1299.5 x (g C2H2/26) = ?
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1. The combustion of acetylene is:
2 C2H2 + 5 O2 4 CO2 + 2 H2O ΔHo = -2511 kJ 11a. (5 pts) How much heat is produced if 85 g
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The problem tells you that you obtain 2511 kJ heat for burning 2*26 or 52 g C2H2. Instead of using
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When 13.0 g of acetylene, C2H2, undergoes complete combustion, 65.5 kJ of heat are released.
a) How much energy is released when
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Mass of one mol C2H2 = 2*12 + 2 = 26 grams/mol (26/12) * 65.5 =131 kJ xC2H2 + (.5 x+2x)O2 ===> 2xCO2
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The flame in a torch used to cut metal is produced by burning acetylene(C2H2) in pure oxygen. Assuming the combustion of 1 mole
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(1251 kJ/mol C2H2) x ? mol C2H2 = 36.658E4 kJ. Solve for ? mols C2H2 and convert to g by g = mols x
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Write a balanced equation for the combustion of acetylene (C2H2). If a reaction consumes 15.9 L of acetylene, how many mol of
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2C2H2 + 5O2 ==> 4CO2 + 2H2O grams C2H2 = volume x density = 15.9 L x 1.097 g/L = 17.4 g mols =
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