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Ammonium nitrate is a common ingredient in chemical fertilizers. Use the reaction shown to calculate the mass of solid ammonium nitrate that must be used to obtain 0.200 L of dinitrogen oxide gas at STP.
A 1.00 g sample of enriched water, a mixture of H2O and D2O, reacted completely with Cl2 to give a mixture of HCl and DCl. The HCl and DCl were then dissolved in pure H2O to make a 1.00 L solution
Draw the major organic product formed when toluene reacts with nitric acid in the presence
A 343 mL container holds 0.146 g of Ne and an unknown amount of Ar at 35°C and a total pressure of 625 mmHg. Calculate the moles of Ar present.
an aqueous solution formed by dissolving 1.62 grams of anhydrous aluminium chloride in 50.0 grams of h2o has a freezing
Compute ΔU for the transformation; a = 0.136 m6Pa mol-2 ; b = 0.0391 L/mol.
Below is the 1H NMR spectrum of the following triazine structure. In the expansions of the spectrum, place the observed multiplicity in the bin above the resonance.
A gas sample has a voulume of 4250 ml at 15 degree celcius and 745mmHg. What is the new container with a voulume of 2.50 L and a pressure of 1.20 atm
How much ice (in grams) would have to melt to lower the temperature of 352 mL of water from 26 C to 4C? (Assume the density of water is 1.0 g/ml.)
What is the certainty in the position of an electron moving at 9.00x10^6 m/s. With an uncertainty of v=0.01x10^6 m/s
How many atoms of iron would be needed to react completely with 36 molecules of oxygen. How many molecules of oxygen would be needed to react completely 16 atoms of iron
Determination of the partial pressures of the gases - Find the partial pressure of each of these gases in the final product mixture.
Each reaction needs to be balanced and all physical states (s, l, g, aq) noted (you may need to look these up or read the lab to determine the physical states).
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