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For the following reaction, if 11.2 L of Nitrogen are reacted to form NH3 at STP, How many liters of Hydrogen will be required to completely consume all of the nitrogen.
N2(g) + 3H2 (g)? 2NH3(g)
Barium metal crystallizes in a body centered cubic lattice. the unit cell edge length is 502 pm and the density of the metal is 3.50g/cm3. using the information, calculate the avogadros number. assume 68% of the unit cell is occupied.
What is the product of toluene+ conj base of alcohol? ( a ring with a O- ) also, where does equilibrium lies?
A mixture containing 2.01 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture.
Compare and contrast the major products of dehydrohalogenation of 2-chloro-4-methylpentane with (a) sodium ethoxide in ethanol and (b) potassium tert-butoxide in 2-methyl-2-propanol (tert-butyl alcohol).
What is the volumetric flow rate of gases out the stack (m3/min)? Note - in these units, R has a value of 0.08206 atm-m3/kmol-K.
Again, are all of the (non-zero) formal charges consistent with the relative EN's of the atoms? Are the structures reasonable?
the energy is 18.44 kj/mol and for the methyl group in equatorial position the energy was 8.66 KJ/mol based on this information which is more stable and why?
Calculate the amount of heat required to completely sublime 14.0 g of solid dry ice (Co2) at its sublimation temperature
A volume of 200mL of nitrogen is collected over water at a temperture of 24 degrees celcius and the atmospheric pressure of 100 kPa. What will be the volume of dry nitrogen at 24 degrees celcius and 125 kPa?
A 1.0 L sample of a gaseous compound of hydrogen, carbon, and nitrogen gave upon combustion 2.0 L of CO2, 3.5 L of H2O vapor, and 0.50 L of N2 (with all gas volumes measured at the same T and P). What is the empirical formula of the compound?
A 3.50-g sample of magnesium hydroxide was treated with 50.0 mL of a 0.500 M aqueous sulfuric acid solution. Calculate the number of grams of magnesium hydroxide that remained undissolved.
An aerosol can has a gas pressure of 138 kPa at 293 K. Calculate the pressure when the can is heated to 506 K.
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