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Alekssandra [29.7K]
3 years ago
13

Aluminum has a density of 2.70 g/cm3. what would be the mass of a sample whose volume is 10.0 cm3?

Chemistry
1 answer:
anastassius [24]3 years ago
3 0
Hey there!

Density = 2.70 g/cm³

Volume = 10.0 cm³

Therefore:

Mass = density *  volume

Mass = 2.70 * 10.0

Mass = 27.0 g
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A compound is found to contain 7.962 % silicon , 20.10 % chlorine , and 71.94 % iodine by mass. to answer the question, enter th
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Empirical   formula  is  calculated   as  follows

calculate  the  moles  of  each  element,  that  is   %  composition/  molar  mass
molar  masses  (  Si=  28.09g/mol ,  Cl=  35.5  g/mol,  I=126.9 g/mol)

moles  of  silicon =  7.962/28.09g/mol=  0.283  moles
moles  of  chlorine =  20.10 / 35.5g/mol =  0.566  moles
moles  of  iodine=  71.94 / 126.9  g/mol=  0.567  moles

divide  each  mole   with  smallest    mole  (0.283)
that  is    silicon =  0.283/0.283= 1 mole
             chlorine =  0.566/0.283=  2 mole
            Iodine=  o.567/0.283= 2  moles
empirical  formula  is  therefore=  SiCl2I2


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2 years ago
How many moles are in an 11mL solution of NaOh and KHP (C8H4O4)​
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Answer:

Calculate the molar concentration of the NaOH solution that you prepared Number of moles of KHP = Number of moles NaOH = 2.476 x 10 -3 moles Number of moles NaOH = Mb x Vb Mb = 2.476 x 10 -3 moles / 0.0250 L (equivalence point) = 0.0990 M 3

Explanation:

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Hello!

The pressure of an 18 L container which holds 16,00 grams of oxygen gas (O₂) at 45 °C is 0,725 atm

To solve this problem we first need to set up the data in the appropriate units to input it in the Ideal Gas Law.

a) 16 g of Oxygen gas to moles of oxygen gas:

16gO_2* \frac{1 mol O_2}{32gO_2}=0,5 mol O_2

b) 45 °C to K

K=$^{\circ}$C + 273,15 = 45 $^{\circ}$C + 273.15=318,15 K

Now, we clear the Ideal Gas Equation for P, and solve it:

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Have a nice day!
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