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Powdered coal ( essentially pure C ) is reacted with excess water to make a mixture of CO,CO2 and H2 The reaction is desired reaction ,CO2 is an undesired waste product. This gas mixture from the reactions of coal with water is further reacted over a catalyst to make methanol (CH3OH)
The Coal is fed with 200% excess water ( excess is calculated with respect to CO formation) 100% of coal is consumed. the selectivity to CO (with respect to CO2) is 1:1 the functional conversion of the CO is 50% what is the final gas composition ? ( all final species are in the gas phase
C+H2O = CO +H2
C+2H2O = CO2 +2H2
CO+2H2O=CH3OH+1/2 O2
The absorbance of a chlorophyll a standard solution in ethanol (density = 0.785 g/mL) is measured in a 1.3 cm cuvette or path length. The absorbance is 0.435 and the molar absorptivity coefficient is 86,300 M-1cm-1. The molecular weight for chloro..
Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 2X -> Y + Z Y + L -> M + Z Part A What is the overall reaction
what is the diameter of an aluminum atom? the mass of 1 mold is 27 g the density of aluminum is 2.7g mol
Calcium Oxide reacts with water in a combustion reaction to producee calcium hydroxide: CaO(s) + H2O(l)----> Ca(OH)2(s)
how many grams of NACL would you need to add to 1 liter water sample ph=7 so that ionic strength equaled to 0.1M
combustion of 1.031g of a compound containing only carbon, hydrogen and oxygen produced 2.265g if carbondioxide and 1.236g of water. What is the empirical formula for the compound?if the molecuar weight is 180.3g, what is the molecular formula?
What is the theoretical yield (in mol) of carbon monoxide when 2.62 mol oxygen reacts with 2.08 mol of ethanol (CH3CH2OH) to produce carbon monoxide and water
An environmental chemist sampling industrial exhaust gases from a coal-burning plant collects a CO2-SO2-H2O mixture in a 21-L steel tank until the pressure reaches 850 torr at 45oC.
A compound contains only carbon, hydrogen, nitrogen and oxygen. Combustion of 0.314 g of the compound produced 0.426 g CO2, and 0.0620 g H2O. In another experiment it is found that 0.103 g of the compound produces 0.0460 g of NH3
In photosynthesis, plants from glucose (C6H12O6) and oxygen from carbon dioxide and water
Sulfuric Acid is the most commonly produced industrial chemical in the world. It is shipped in a concentrated form to save volume and weight.
C2H4(g) + H2O(g) C2H5OH(g) 1 mol C2H4, 1 mol H2O at 355K and 1 bar. Using equilibrium constant approach, calculate the equilibrium extent of reaction and the mole fractions
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