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The complete combustion of acetylene (C2H2), the fuel used in acetylene welding torches, produces carbon dioxide gas and water vapor and releases 1256 kJ of heat energy per mole of acetylene.
a. Write out the complete balanced thermochemical equation for this reaction.
b. How much heat in J will be given off by the complete reaction of 25 mL of acetylene? (1 mL = 1 cm3 , density of acetylene = 1.097 g/cm3 )
c. How much acetylene must be burned to produce enough heat to melt 27.5 g of iron? Assume the iron is already at its melting point of 1539°C . (Hfus of Fe is 13.8 kJ/mol)
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At 25 °C, water has an equilibrium vapor pressure of 23.8 mm Hg. If 2.500 g of water is sealed in an evacuated 10.0-L flask and heated to 25 °C, what mass of water will evaporate?
This was a question on my Mastering Chemistry homework. It's from Tro's Cha: Determine the pH of the following two-component solution: 0.260 M NH4NO3 and 0.102 M HCN
an aqueous solution formed by dissolving 1.62 grams of anhydrous aluminium chloride in 50.0 grams of h2o has a freezing
how many different alkenes will be produced when each of the following substrates is treated with a strong base? a) 1-Chloropentane
6.48g of NAH2PO4 and 21.96 g of K2HPO4 are dissolved in sufficent water to make a liter of solution. Caluclate the ph of the resulting solution.
say you removed an ice cube at -10 ordmc weighing 36 g from your freezer. now you place the ice cube in a 90 g sample
Explain how would I find the percent yield and what would it be if I have 3.292 g of p-anisaldehyde to start out with, 2.905 g of acetophenone needed for the reaction between p-anisaldehyde and acetophenone, as well as 4.151 g of recovered trans-..
Calculate the volume of ammonia required to bring the pH to 3.00 and to 8.00. Kb (NH3) = 1.8 x 10^-5.
The overall equilibrium involves Ksp, Ka3 of phosphoric acid and Kw. Construct the constant and show the three equations that apply.
The following values of saturation drain current (ID,sat) were collected from several test wafers with a sample size of n = 5.
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