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Anton [14]
3 years ago
10

Suppose you take a solution and add more solvent, so that the original mass of solvent is doubled. you take this new solution an

d add more solute, so that the original mass of the solute is doubled. what happens to the molality of the final solution, compared to the original molality?
Chemistry
1 answer:
ser-zykov [4K]3 years ago
3 0
The molarity remais the same
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1.1214 mL will a 0.205-mole sample of He occupy at 3.00 atm and 200 K.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Using equation PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

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Putting value in the given equation:

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brainly.com/question/27691721

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To calculate the mass of Fe formed in a) we get first the limiting reactant between Fe2O3 and CO. Given the masses, the ratio of Fe2O3 is 1.33 while that of CO is 1.67. Hence the limiting reagent is Fe2O3. The mass of Fe formed is 148.98 grams. In b, the needed CO is only 112.04 grams. Hence, the excess is 27. 96 grams. 
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