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To find the number of moles in I2, we have to know the atomic weight of iodine (which my Periodic Table tells me is 127). But iodine is a diatomic element, existing in molecules of 2 iodine atoms bound together (I2). So the molecular weight of I2 is 2 x 127 = 254g/mole.
Moles = mass/MW, so moles = 450g/(254g/mole). The "grams" cancel out and the answer is 1.77 moles.
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How will intensity of maxima and minima in youngs double slit experimentchange if one of slit is covered by a transparent paper which transmits only half of light intensity?
The intensity of the maxima and minima in Young's double slit experiment will decrease by half when one of the slits is covered by a transparent paper that transmits only half of the light intensity. This is due to the reduced amount of light passing through the slit, resulting in a weaker interference pattern with lower contrast between the bright and dark fringes.
Consider two long straight parallel wires each carrying a current I. If the currents move in the same direction?
The magnetic fields produced by the two wires will reinforce each other, creating a stronger magnetic field between them. This results in an attractive force between the wires. The force is given by the formula F = (μ0 * I1 * I2 * L) / (2πd), where μ0 is the permeability of free space, I1 and I2 are the currents, L is the length of the wires, and d is the distance between the wires.
What is the formula for calculating power in a circuit using the keyword "power i 2r"?
The formula for calculating power in a circuit using the keyword "power i 2r" is P I2 R, where P represents power, I represents current, and R represents resistance.
What is the formula for calculating power loss in a circuit, involving the keyword i2r?
The formula for calculating power loss in a circuit is P i2 R, where P represents power loss, i is the current flowing through the circuit, and R is the resistance of the circuit.
What is the formula for calculating power loss in transmission lines?
The formula for calculating power loss in transmission lines is Ploss I2 R, where Ploss is the power loss, I is the current flowing through the transmission line, and R is the resistance of the transmission line.
What is the number of moles in 12.7 grams of iodine?
For this you need the atomic (molecular) mass of I2. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. I2=253.8 grams12.7 grams I2 / (253.8 grams) = .0500 moles I2
How many grams of I2 should be added to 750 g o C Cl4 to prepare a 020 m solution?
To prepare a 0.20 M solution of I2 in CCl4, you would need to calculate the moles of I2 required first. Molarity (M) = moles of solute / liters of solution. Since you know the molarity and volume of the solution, you can calculate the moles of I2 required and then convert that to grams using the molar mass of I2.
What are 25.4 g of iodine and 14.2 g of cl made to react completely to yield a mixture of icl and icl3 cal the no of moles of icl and icl3?
I2 + 2Cl2 .==> ICl + ICl3 molar mass of I2 = 127 molar mass of Cl2 = 70.9 moles of I2 used = 25.4/127 = 0.2 moles of I2 moles of Cl2 used = 14.2/70.9 = 0.2 moles of Cl2 Since the stoichiometry indicates that each mole of I2 reacts with 2 moles of Cl2 to give 1 mole each of ICl and ICl3, you should get 0.1 moles of each product. The reason you don't get 0.2 moles is because the amount of I2 is limiting, and you can see that 2 moles of Cl2 will use up 1 mole of I2, so 0.2 moles of Cl2 will use up 0.1 moles of I2. So 0.1 moles of product is all you can get under these conditions
How many grams of iodine are produced when 0.72 mol of fluorine reacts with potassium iodide KI 2 KI F2 -- 2 KF I2?
From the balanced chemical equation, 2 moles of potassium iodide (KI) react with 1 mole of fluorine (F2) to produce 2 moles of iodine (I2). Therefore, when 0.72 mol of fluorine reacts, it produces 0.72 mol/2 = 0.36 mol of iodine. To convert this to grams, you would multiply the moles by the molar mass of iodine (I2), which is approximately 253.8 g/mol. So, 0.36 mol * 253.8 g/mol ≈ 91.4 grams of iodine are produced.
How much energy is needed to melt 25.4grams of l2?
To calculate the energy needed to melt 25.4 grams of I2 (iodine), you can use the formula: energy = mass x heat of fusion. The heat of fusion for iodine is 15.52 kJ/mol. First, find the molar mass of I2 (253.8 g/mol) and then convert the mass to moles. Finally, multiply the moles by the heat of fusion to get the energy needed.
How many molecules are in 110g of iodine gas (I2)?
To find the number of molecules in 110g of iodine gas (I2), we first need to calculate the number of moles. The molar mass of iodine gas (I2) is approximately 253.8 g/mol. So, 110g is equivalent to 110/253.8 ≈ 0.43 moles of I2. One mole of a substance contains 6.022 x 10^23 molecules (Avogadro's number), so 0.43 moles of I2 contains about 0.43 x 6.022 x 10^23 = 2.59 x 10^23 molecules.
What quantity of iodine can be obtained if 20.0 g of NaI is mixed with 10.0 g of MnO2 and treated with a stoichiometric excess of sulphuric acid?
The balanced chemical equation for this reaction is: 2NaI + MnO2 + 2H2SO4 -> 2NaHSO4 + MnSO4 + 2H2O + I2 From the balanced equation, 1 mol of NaI gives 1 mol of I2. First, find the number of moles of NaI and MnO2, then determine the limiting reactant. Finally, calculate the moles of I2 formed based on the limiting reactant and convert to grams using the molar mass of I2.
How many moles of iodine molecules correspond to 1.80x1024 molecules of I2?
To find the number of moles, you first need to determine the molar quantity of iodine molecules based on Avogadro's number. Since 1 mole contains 6.022 x 10^23 molecules, you would divide 1.80 x 10^24 molecules by Avogadro's number to get the number of moles.
How many moles in 135 g of iodine?
not sure
What is the stoichiometric relationship between IO3- and I2?
The iodine content ratio of IO3- and I2 is 1 to 2
Equal weight of Zinc metal and Iodine are mixed together and the Iodine is completely converted to zinc iodide What fraction of weight of the original Zinc remains unreacted?
Balanced equation is: Zn(s) + I2(s) --> ZnI2(s) Pick any initial mass of Zn and I2, and convert those masses to moles: 100 g Zn / 63.4 g/mol = 1.58 moles 100 g I2 / 253.8 g/mol = 0.394 mol I2 Since these two react in a 1:1 ratio, you will have used 0.394 moles of Zn to react with the 0.394 moles of I2. That would leave 1.58 - 0.394 = 1.186 moles of Zn unreacted. So, the fraction of the original zinc remaining would be 1.186 / 1.58 = .75 by sonu gupta
How do you make 1 liters of 0.02 N iodine solution?
To prepare 1 liter of a 0.02 N iodine solution, first calculate the amount of iodine (I2) needed. Since the normality of the solution is based on the equivalent weight of iodine, and considering that 1 equivalent of iodine corresponds to 1 mole of I2, you need 0.02 equivalents in 1 liter. This translates to 0.02 moles of I2, which is approximately 5.12 grams (molar mass of I2 is about 253.8 g/mol). Dissolve this amount of iodine in enough distilled water to make a final volume of 1 liter.
