1) The fertilizer ammonium sulfate (NH4)2SO4. is prepared by the reaction betwee

Question

1) The fertilizer ammonium sulfate (NH4)2SO4. is prepared by the reaction between ammonia (NH3) and sulfuric acid:

     2NH3(g)+H2SO4(aq)----->(NH4)2SO4(aq)

How many kilograms of NH3 are needed to produce 2.10*10^5kg of (NH4)2SO4? (scientific notation).

2) Nitroglycerin (C3H5N3O9) is a powerful explosive its decomposition may be represented by

    4C3H5N3O9--->6N2+12CO2+10H2O+O2

this reaction generates a large amount of heat and gaseous products. It is the suggen formation of these gases, together with their rapid expansion, that produces the explosion.

(A) What i the maximum amount of O2 in grams that can be obtained from 2.50*10^2g of nitroglycerin? (g)

(B) Calculate the percent yield in this reaction if the amount of O2 generated is found to be 7.87g. (%)

3) When potassium cyanide (KCN) reacts with acids a deadly poisonous gas, hydrogen cyanide (HCN) is given off

     KCN(aq)+HCl(aq)--->HCN(g)+KCl(aq)

If a sample of 0.380g of KCN is treated with an excess of HCl, calculate the amount of HCN formed in grams.

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Explanation / Answer

1) moles of (NH4)2SO4 = 2.1 x10^ 8 gm/ 132.14 = 1.589 x10^ 6 ,

moles of NH3 = 2 x 1.589 x10^ 6 = 3.17845 x10^ 6 ,

mass of NH3 = 3.17845 x10^6 x 17 =5.4 x10^ 7 gm = 5.4 x10^ 4 kg

2) A) moles of nitroglycerine = 250 /227 = 1.10132 , moles of O2 = 1.1032/4 = 0.2753,

amount of O2 = 0.2753x32 =8.81 gm,

B) % yiled =(7.87/8.81) x100 = 89.33 % ,

3) moles of KCN = 0.38/65.12 = 0.005835 ,moles of HCN = 0.005835,

mass of HCN = 0.005835 x27 =0.1575 gm

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