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| i need help with this physics problem |
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Posted by: MyCredit2018 - 01-17-2020, 12:35 AM - Forum: aluminium faq
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i have a homework to do and its about Heati have answered it already but i need to be sure if its correct.q: By accident, 20g of aluminum at 275°C is dropped to a 25g of water at 80°CHow much steam is produced? anyone knows the solution for this problem?please use the equation QmLvwhere, Q - heat m - mass Lv - heat of evaporation 2.25x10^6 J/kgthanks!!!!The heat leaving the aluminum all goes into heating the water from 80C to 100C and then evaporating x grams of water: M_alu C_alu (275 - 100) M_water C_water 20 + x Lv Solve for x: x ( M_alu C_alu (275 - 100) - M_water C_water20) / Lv (20g 0.897 J/(g C) 175C - 25g4.18J/(g C) 20C) / (2.2510^3 J/g) 0.47 gramOther related question
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| Heat Capacity Question CHEM |
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Posted by: AimeeCyday - 01-17-2020, 12:35 AM - Forum: aluminium faq
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A 100.0g sample of aluminum is heated to 100.0 oC (Celsius) and is placed in a coffee cup calorimeter containing 150g of water at 25.0 oCAfter the metal cools, the final temperature of the metal and the water is 34.1 oCCalculate the specific heat capacity of aluminum from these experimental data, assuming that no heat escapes to the surroundings or is transferred to the calorimeterSpecific heat of water 4.184 J/g oCatomic mass Al 27.0 g/molCalculate your answer in J/g oC with 3 significant figures, but enter the answer without units.Then calculate the molar heat capacity of Al in J / mol oC, again, to 3 significant figuresEnter the answer without units.The heat given off from aluminum (from initial heating) will eventually equal the heat energy absorbed by the water at the final temperature, 34.1 oCqAl qWater q m.c.deltaT (100.0g Al)(X J/g oC)(100 - 34.1) (150.0g H2O)(4.184 J/goC)(34.1 - 25.0) Solve for X, specific heat capacity of aluminum 6590X 5711.16 X 0.867 J/g oC Al The molar heat capacity in J/mol oC Molar mass x specific heat Al 27.0g/mol x 0.867 J/g oC grams cancel, leaving J/mol oC 23.4 J/mol oCOther related question
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| Advice regarding FIMO modelling clay |
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Posted by: Josephicexy - 01-17-2020, 12:35 AM - Forum: aluminium faq
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I am working on a small project using FIMOI have made it into the shape that I require but the trouble is it is stuck to the item that it will eventually be attached toThe FIMO is too thin to be able to peel it off without it breaking upI need to somehow cure the FIMO so that I can remove it but I cannot put this item into the oven as it is made of plastic/vinyl materialI am currently using a hairdryer to heat parts of it for a short time without melting the object it is attached to, is this the best way to do it? Even if I was able to remove the FIMO from the object, it wouldn\'t be possible to support it well enough in an oven without the shape becoming distorted.The hairdryer seems like the easiest choice and I think that this should work since the FIMO is thinBut also try a heat gun, but I understand there\'s a chance to damage the plastic item And another idea is is you can peel off the FIMO, then you can create a support to hold its shape while bakingTo do this, crumple up some aluminum foil and try to re-create the shape of the plastic item, then transfer the FIMO into thisYou might need to re-sculpt any tears as you transfer to the foil.Other related question
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| do floating tealights in glass bowls make the glass bowls crack |
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Posted by: dtaletktqk - 01-17-2020, 12:35 AM - Forum: aluminium faq
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I tired putting tea lights in a glass fish bowl full of water and the tea light flame was on the edge of the glassa few minutes later it crackedis this from the heat? is it just cheap glass? would thicker glass be better? Is it that the bowl was too full? It was about 3/4 fullDoes anyone have any remedies? I am using this idea for my wedding.the heat difference of heat at the bowl make the crack .like you put hot water in chill glass .even if you put the thick glass this will crack .so better put water proff under water light in the bowl which you can find in aqua: shop with 12/24 DC voltageOther related question
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| What is the best way to clean sterling silverwhile at home |
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Posted by: luzxf2 - 01-17-2020, 12:35 AM - Forum: aluminium faq
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What type of solvents can I use to take of dirt and residues.Thanks so much for your time and information.Sincerely,Tom ScienceThe gentlest way I know involves heating it gently in a large pan of water (not an aluminium pan) with some baking soda dissolved in ithe water and some crumpled up aluminium foil Best of luck - MikeOther related question
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| Reaction between aluminum and Im not sure what else |
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Posted by: GlennisRab - 01-17-2020, 12:35 AM - Forum: aluminium faq
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Okay, so I was one of four people in my AP chemistry class today because of a different AP test most of the class was out forNaturally, we all went to the lab and got to do cool things we wanted toI read instructions and managed to coat several pennies in brass, using a mixture of the two pennies, zinc metal, and sodium hydroxideThis mixture was heated and the pennies were coated in zincThen, the pennies were heated in a flame and the outer zinc layer mixed with the copper already there and presto, the pennies were coated in shiny brassAnyway, when I was all done, I added a little piece of aluminum foil to the mixture to see if anything would happenIt bubbled violently and released a gas that burned the inside of my noseI\'m just wondering, what exactly did the aluminum react with? I know a reaction is supposed to occur with sodium hydroxide, but is it supposed to be this violent? And it could also have occurred with the copper (II) ion dissolved in solutionAnyone know what happened?The gas evolved was H2 and the bubbles carried along some of the alkaline solution which would account for the burning sensationAluminum placed in NaOH solution is an excellent way to generate small quantities of hydrogen gas and the reaction is vigorousSome of the copper ions might have cleaned the surface of the Al aiding in the attack of the hydroxide ion on the Al metal surfaceEven water will evolve hydrogen with aluminum if the surface is clean2 Al + 6 H2O + 2 NaOH - 3 H2 + 2 NaAl(OH)4Other related question
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| Where to purchase Walther P38P1 barrel and frame |
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Posted by: DebbieFoss - 01-17-2020, 12:35 AM - Forum: aluminium faq
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Just purchased a very nice Walther P1/P38 and it\'s in great shapeI can rebuild it with the Walther kit of parts with slide, grips and partsHowever, no barrel or frame is includedAny help ?The frame has the serial number and is considered the firearmP38 and P1s have different framesThe P38 is steel and the P1 is anodized aluminumIf it\'s in great shape why do you want to rebuild it?Other related question
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| How many moles of Al ions and O ions does 04 mole of aluminium oxide have |
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Posted by: PeterElepe - 01-17-2020, 12:35 AM - Forum: aluminium faq
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Plz help me with these following questions as well.I\'ve been trying to get the right answers for so long but i can\'t find it.but I do have the answers of the questions.what i need is the steps.2.What is the mass of 2.3 moles of aluminium oxide?3.What is the molar mass of tetrachloromethane, CCl4?4.How many moles of aluminium ions are present in 17.12g of aluminium sulphate?5.What is the formula mass of iron(II)Sulphate-7-water, FeSO4 7H20?I really need help in these questions.ThxThe formula Al2O3 means that 1 mole of Al2O3 has 2 moles of Al ions and 3 moles of O ionsSo, any sample of Al2O3 will always have a 2 to 3 ratio of Al and OIn your 0.4 mol of Al2O3, there are 0.8 mol of Al ions and 0.12 mole of O ions since 0.8 to 0.12 is a 2 to 3 ratio 2.3 mol times 101.961 g/mol 234.5103 g rounded off to two sig figs, the answer is 230 g one C + 4 Cl 12 + (4) (35.5) 154 g/mol Using better numbers gives 153.823 g/mol Al2(SO4)3 convert 17.12 g to moles by dividing by the molar mass of Al2(SO4)3 multiply moles by 2 Get a periodic table to look up atomic weights FeSO4 7H20 one Fe one S four O 7 H2O (H2O 18.015, after awhile one gets that value memorized) Add them upThe dot between the FeSO4 and the 7H2O is not a multiplication dot.Other related question
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