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Ammonium nitrate is a common ingredient in fertilizers that can also be used to make explosives because it decomposes as follows:
NH4NO3(s) ? 2 N2(g) + O2(g) + 4 H2O(g) ?H = -236 kJ
The following questions deal with the decomposition of 12.1 g of NH4NO3:
(a) How much heat is liberated under standard conditions?
(b) How much work would be done by the gases at 310.°C?
(c) What volume of gas would be produced at 1.05 atm pressure and 310.°C?
if the initial water level in the graduated cylinder is 21.2 ml and the level rises to 27.7 ml after the object is placed in the cylinder, what is the volume of the object?
You burn 0.0956 g of the compound and isolate 0.1356 g of CO2 and 0.0833 g of H2O. What is the empirical formula of the compound.
A titration experiment is set up to use .235M bleach (NaOCl) to analyze CrO2^-. If 50mL of the CrO2^-(aq) solution required 28.62mL of bleach to react to completion, what would you calculate as the molarity of the CrO2- solution
CO(g)+2H2(g)->CH3OH(g) How many moles of each reactant are needed to produce 3.60 X 10^2g of CH3OH?
0.134 mole of kcl and 0.248 mole of cacl2 were dissolved in water. calculate the total number of moles of cl- ions in the solution.
what percentage of the acid is not ionized? (Assume all H in solution came from the ionization of HA.)
Calculate the volume of carbon dioxide at 20.0 C and .960 atm produced from the complete combustion of 3.50 kg of methane. Compare your result with the volume of CO2 produced from the complete combustion of 3.50 kg of propane (C3H8)
The two products formed are 2-methyl-1-hexene (19%) and 2-methyl-2-hexene (81%). Show the chemical equation for this reaction. Explain fully why 2-methyl-2-hexene is the major product.
What is the percent yield of a reaction in which 238 g phosphorus trichloride reacts with excess water to form 143 g HCl and aqueous phosphorus acid (H3PO3)?
Determine the volume of the sample. (b) Plot the data. Now suppose you add another 5.00 mol of gas molecules into the same volume.
A student dispensed 20.00 mL of 2x10^-5 M blue #1 solution into a test tube. He then added 2.00 mL of NaCl solution and 2.00 mL of 2.50 % bleach solution.
Why is a solution of sodium bisulfite added to the reaction product mixture? Write a reaction to account for what is happening
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