Empirical formula for acetic acid
The empirical formula for acetic acid is CH2O. Its molar mass is 60 g/mol. The molecular formula is
A. C2H4O2
B. C2HO2
C. none of the above
D. CH2O
E. C2H6O
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Carbon monoxide and water vapor, each at 200. Torr, were introduced into a 250. mL container. When the mixture reached equilibrium at 700.°C, the partial pressure of CO2(g) was 88 Torr. Calculate the value of K for the following equilibrium.
The filtrate after the removal of the black precipitate was basified with 6M ammonia. This when treated with 3M ammonium carbonate, it gave a white precipitate. This white precipitate was dissolved in 6M acetic acid and basified with ammonia(6M).
Why is the internal-standard method often used in plasma emission spectrometry?
The average pH of precipitation in rural areas is 7.00. Assuming that the pH is controlled by the carbonate system, i.e., no anthropogenic acid gases are present in the atmosphere.
A certain first-order reaction () has a rate constant of 7.50×10-3 at 45 . How many minutes does it take for the concentration of the reactant, to drop to 6.25 of the original concentration?
In the reaction between potassium carbonate and calcium nitrate (balanced eq: K2CO3 + Ca(NO3)2--> K2(NO3)2 + CaCO3), why wouldn't ...--->2KNO3 +CaCO3 be right?
Consider the following reaction, equlibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g)
Phosphorus pentachloride, PCl5, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of PCl5.
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