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A: Please find your solution below : Melting point of any substance is defined as the temperature at…
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A: Examples of silicates: Quartz, feldspar, mica, amphibole, pyroxene, and olivine. Silica tetrahedra.
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A: Silicon * Silicon is a naturally occurring chemical element. * It acts as metalloid that is it…
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A: Particles with a size below 1 × 10-9 m ( 1 nanometer ) are called as nanoparticles or nanomaterials.…
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A: Nanocarbons are carbon-based nanomaterials, and have unique physico-chemical properties.
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A: There are various methods through which Cobalt(II) sulfate heptahydrate (CoSO4. 7H2O) can be…
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A:
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A: The reaction of barium hydroxide and sulfuric acid is:
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A: Samples A= Fullerenes+ C16 to C70B = Nano diamondC = C60+carbon nanotubesD = graphite+ graphene
Q: of KClO3 that decomposed.
A: Volume of oxygen = 52.4 mL = 52.4/1000 = 0.0524.L Pressure of Oxygen = 765.2-22.6 = 742.6 mm Hg…
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A: Solutions- Crystals are hydrated because water molecule in present inside the crystal.
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A: Note : All hydrated are discussed here.
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A: a) Hydrogen bondingis a special type of dipole-dipole attraction between molecules. It results from…
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Q: c) What is the oxidation state of xenon in XeO4 and XeF6. (Show your work)
A: The Xe element belongs to the noble gas family. The noble gases are inert in nature.
Q: Describe how the following changes are brought about: (i) Pig iron into steel. (ii) Zinc oxide into…
A: ( i ) Pig iron into steel: Pig iron is charged into basic oxygen furnace (BOF) and water cooled…
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Q: Why is Cl2 a gas, Br2 a liquid, and I2 a solid at room temperature?
A: In non-polar molecules, London dispersion forces occurs. These types of forces are directly…
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A: Molar mass of BaSO4 = 233 g/mol Molar mass of sulfur = 32.0 g/mol 1 mole of BaSO4 contains 233 g and…
Q: silicates
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Q: Complete the balanced equation for the reaction of calcium with water. Write the missing product in…
A: Calcium Ca Water H2O Hydrogen H2 Calcium hydroxide Ca(OH)2
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Q: a sample of KClO3 (Mw = 122.55 g/mol) allowed to decompose in presence of MnO2. The resulting oxygen…
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Q: Which has the highest melting point? LiH, CH4, or NH3
A: Melting point of the substance is the temperature at which it start to melt and at the melting point…
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Q: what substance is formed when water is added to metallic oxide? how will you prove this?
A: Metallic oxide reacts with water and gives metal hydroxide.
Use your knowledge of formation of ionic compounds and the cross over method. Show how Ca3(PO4)2 and CaCO3 were formed. Show your working
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- Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the average molecular mass for this sampleChlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 1.43 g/L at 26 °C and 0.405 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of CH2F2 in the sample.Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111-trifluoroethane (C2H3F3) has a density of 2.39 g/L at 23 °C and 0.593 atm. 1. Calculate the average molecular mass for this sample. 2. Calculate the volume percentage of C2H3F3 in the sample.
- Acetylene had many uses at the time of the First World War, because it burned with a hot and luminous flame mainly. The oxyacetylene apple and the period of the oxyacetylene car company and bicycles made this good represent well. In an attempt to find a route to acetylene other than through calcium carbide, a Prest-O-Lite sponsored research by George O. Curme of the Mellon Institute in Pittsburgh. Ethylene research was directed towards converting gases for refining petroleum methods, led to more polyethylene material for acetylene production. Viewed from today's perspective, the Curme route to petroleum-based ethylene ranks as an important discovery. However, this was not the case at the time, because ethylene had almost no use before 1920. Curme's second major contribution was the research he carried out to see what useful products he could make with ethylene. The first was ethylene glycol, which became Prestone antifreeze. Others follow and now ethylene is evidently the most…The production of cement results in significant GHG emissions. The emissions are caused by the decomposition of calcium carbonate (limestone) to calcium oxide (lime) and carbon dioxide. This process known as calcination, is carried out in kilns. Therefore, additional GHGs are emitted as a result of heating the kilns. A large cement manufacturer uses a mix of coal, natural gas, and biomass in its boiler. This mix produces the following amounts of GHGs per Million BTUs of energy: • 250 lbs CO2/MMBtu • 5 lbs CH4/MMBtu • 0.36 lbs N2O/MMBtu Process carbon emissions from the calcination process produce 925 lbs of carbon dioxide per metric ton of cement. In addition, the plant uses 1.7 Million BTUs of energy per metric ton of cement. If the plant produces 180,000 metric tons of cement annually, how many metric tons of CO2e does it emit?A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹
- A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!Meztiza, a beer cocktail, is prepared by mixing rum, beer, and cola. Compute the finalconcentration(%w/v) of ethanol in meztiza if 100.0 mL of beer was first mixed with 5.0 mL rum andbefore finally diluting it with cola to produce 200.0 mL of the beer cocktail. ( a beer contains about 4.50% (v/v) of ethanolfermented by yeast from sugars while rum contains about 40.0% (v/v) ethanol. Meanwhile, arubbing alcohol is also an alcohol solution which contains 70.0 %(v/v) isopropyl alcohol fermentedby a bacterium instead of a yeast)0.1 g of a sample of coal was used in a bomb calorimeter for the determination of calorific value. The ash formed was extracted with acid and the acid extract was heated with BaCl2 solution and a precipitate of BaSO4 was obtained. The precipitate was filtered, dried and weighed. The weight of precipitate was found to be 0.01 g. Calculate the percentage of sulfur in the coal sample.
- 2N2(g) + 3O2(g) ® 2N2O3(g) (delta)H°rxn = +86.6 kJ Consider a reaction mixture of 13 grams of 7N and 17 liters at STP (LSTP) of O2: … If all 13 grams of 7N react, the reaction heat is: _________ kJ … If all 17 LSTP of O2 react, the reaction heat is: _________ kJ … The limiting reagent in this mixture is _____ … The theoretical heat of this reaction mixture is: _______ kJ19. Solid urea, (NH2)2CO, burns to give CO2, N2, and liquid H2O. Its heat of combustion is -632.2 kJ/mol. 1.Write the balanced combustion equation. Record fractions as ratios (e.g. 1/2) if needed. Include aggregation states in your answer. 2.Calculate the heat generated per mole of H2O formed to 0.1 kJ. 3.Using this heat of combustion and the appropriate thermodynamic data, determine the heat of formation of urea to 0.1 kJ.A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0125 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.4ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.