what is the freezing and melting point of a bimetallic strip?
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A bi-metallic strip is used to convert a temperature change into mechanical displacement. The strip consists of two strips of different metals which expand at different rates as they are heated, usually steel and copper.\n\nThe copper melting point is (1084.62 °C, 1984.32 °F)\nSteel often melts at around 1370 degrees C (2500°F).\n\nIt doesn't have a freezing point because it's a solid.
16969
It's a solid, so it's already frozen. Heat it up enough, and it will melt.
623583
answer can be a or c, but i'd go with answer c.\n\nthe melting point (which solid becomes liquid) varies by each molecules & substances.  What happen is when temp. rises, it translates into more energy put into the soild or heat absored by the solid.\n\nHowever, you can melt solid by chaning pressure, and leaving temp constant.\n\nSo best answer would be C, by heat absorption.
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Ice melting\nWater freezing\nWater boiling\nAmmonium chloride subliming
1014247
there are different tempuratures to melt gold and copper,for instance gold is a softer metal and it will melt before the copper.say the temp for melting gold is 1000 degrees,and copper is 1200 degrees,the gold will melt first.
1072945
Gold melts at 1945 ° F or 1063 ° C...
226408
the question as written has no answer.  hydronium is an ion that only exists in a solution, never by itself. so it can't have a melting point or freezing point or a density
5530
Arsenic is the metal, but at temperatures much lower than its melting point (not boiling point).  It sublimes at 614 degrees C and melts under pressure at 817 degrees C.\n\nAlthough Iodine has a metallic luster, it is not a metal.  It sublimes (evaporates) near its \nMelting Point of 114 degrees C.\n\nSee the reference below:
125282
Most efficient? If you don't have a lab, then I would assume just doing your best at grinding off the top layer, and trying to melt the shreddings down into a >70% gold alloy. Since gold's melting point is OVER 1000 degrees Celsius, I suppose your best bet is to heat the grindings as much as possible, and then pounding them together into a single mass (like a black-smith...or 'gold-smith'). But you have to realize HOW LITTLE gold is actually on there. The layer is so thin...sometimes merely 2-3 micrometers. You're gonna get a lot of impurities, such as nickel and copper. Gold-plating is usually done on copper or silver; and in the case of copper, a thin layer of nickel is placed below the gold. And since the melting point of nickel isn't that far from that of gold, and copper's is almost EXACTLY that of gold's, you're gonna get a random mixture of crap. I imagine the process is more trouble than it's worth. I'd just go buy gold from alfa aesar or somewhere like that for cheap-as-free.
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One method is using bimetallic strips of metals that can stand very high temperature. Bimetallic strips bend when the temperature changes.
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I would need more information to help you answer that question.\n\nWhat is the mass of the metal being used? What was the original temperature of the metal?\n\nThe formula you need is:\n\nq = mc(Tf - Ti)\n\nq = energy change\nm = mass\nc = specific heat\nTf - Ti = change in temperature
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Have each page work on the same princable as the bi-metallic thermometer.  Try to find two materials the expand differently than eachother because of heat, or you could use humidity to expand one material more than the other. You could probably find some material that contracts (or expands) when an electrical current passes through it. place a strip of this along the top and bottom of each page. Thats all i can think of right now.\nCool question by the way.
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Titanium melting point = 1675 C, boiling point = 3260C, so at NPT it is a metal, and will be insoluble in anything other than dilute acid (CRC, physical constants of inorganic compounds).
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malleable and ductile lustrous conduct heat and electricity high melting points almost all are solids at room temp except mercury
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Solid in room temp, but melts in your hand (slightly above room temp)\n\nAlloys quickly with most metals.\n\nYou can read more at the following:
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If you were able to get the salt solution cold enough, it would freeze. However, if you put two ice trays side by side, one filled with water, the other filled with salt water, and chilled them to the point where both froze, the would both be the same temperature. However, once the cold was taken away, the salt solution would melt at a much lower temperature than the water only cubes.\n\nWhat salt does when added to water is decrease the temperature at which water will freeze -- as well as melt. How much the freezing/melting point is lowered depends on how much salt is added. The higher the concentration, the lower the freezing/melting point.
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It's because of the lower pressure with the higher altitude.  Remember the phase diagram denotes the phase of a particular compound in terms of the pressure and temperature.  If you're sufficiently talented with respect to the maths, refer to a physical chemistry text and research upon chemical equilibrium and dG/dn.\n\nhttp://www.freewebs.com/chemistryhomework\n\nEDIT:  \n\nYou said:\n------------\nThe phase diagram doesnot explain this.\nYou forgot that it takes higher pressure to shift the freezing point higher in the phase diagram, not lower pressure like up in the mountain.\n--------------\n\nIncreasing the pressure makes it easier to melt ice, e.g. the pressure exerted by ice skates result melted ice at the surface, this is a common excerpt in introductory chemistry texts.  Again, also consider dG/dP and chemical equilibrium.