Titanium(Ti)
1 mol = 6,022 x 10^23 molecules of HI. So: 6,022E23 *0,3 = Your answer !
Titanium, atomic number 22 with an Atomic Mass of 47.867 amu, is represented with the symbol Ti.
Take 1.45 wt% oxide as an example. To remove the oxide component first you must work out the Ti component: 1.45 wt% oxide x 0.6 = Ti (wt%) because Ti in TiO2 makes up 60% its formula mass: 47.87 / 79.87 = ~0.6 Ti Thus 1.45wt% TiO2 = 0.87 wt% Ti
IU is not a measurement of mass or weight like others but ti is the measurement of potency of a drug such as...vitamin capsules. =)
6.022 x 1023= 6.022e+23
65.39 grams titanium (1 mole Ti/47.87 grams)(6.022 X 1023/1 mole Ti) = 8.226 X 1023 atoms of titanium -------------------------------------------
Not easy to do in your head. 210 = 1024, 29=512, so 229 will be 1024 * 1024 * 512. REALLY rough estimate is 1000 * 1000 * 500 = 5 with 8 zeros. 500,000,000. My TI-84 Silver Edition tells me it is really 536,870,912.
Titanium(Ti)
1 mol = 6,022 x 10^23 molecules of HI. So: 6,022E23 *0,3 = Your answer !
Titanium, atomic number 22 with an Atomic Mass of 47.867 amu, is represented with the symbol Ti.
Titanium (Ti)
Titanium chloride is TiCl. You must convert those grams given to you into moles first. So you have .311 g Ti and .689 g Cl. So.... to convert to moles: for Ti: find the molar mass of Ti. This is 47.90g/mol. 0.311g Ti x 1 mol Ti/47.90g/mol Ti= .006mol Ti For Cl: The molar mass of Cl is 35.45g/mol. 0.689g x 1mol Cl/35.45g/mol= .019mol Cl So you've got 0.006mol Ti and 0.019mol Cl. Now you have to divide both by 0.006 to get the empirical formula. So: 0.006/.006= 1mol Ti .019/.006= 3mol Cl Your empirical formula would be TiCl3
Ci is not a known chemical element: please rephrase the question. Possible: Cl (chlorine) Cu (copper) C (carbon), Ca, Cd, Cr, Cs, Ce, Co, or Si, Ti, Bi, etc. There are too many possibles.
Mass number of Titanium = 46 Atomic number of titanium = 22 = number of protons present Mass number = No. or protons + number of neutrons So number of neutrons = 46 - 22 = 24
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Take 1.45 wt% oxide as an example. To remove the oxide component first you must work out the Ti component: 1.45 wt% oxide x 0.6 = Ti (wt%) because Ti in TiO2 makes up 60% its formula mass: 47.87 / 79.87 = ~0.6 Ti Thus 1.45wt% TiO2 = 0.87 wt% Ti