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Vedmedyk [2.9K]
3 years ago
7

When placed in a 100-mL square box, a substance has a spherical shape and has a volume of 50 mL. When placed in a 100-mL circula

r tube, that same substance has a spherical shape and a 50-mL volume. In what phase or state was the substance?
Chemistry
1 answer:
ikadub [295]3 years ago
8 0

Solution: There are major three phases of substance, namely solid, liquid and gas.

Here, solid substances have definite shape, they are rigid and can not change their volume or shape if kept in any container.

Liquid substances do not have any shape of their own, they take shape of the container in which they are kept. They are compressible in nature.

Gaseous substances also do not have their own shape, the molecules of gas continuously move in the container in which they are stored. Gases are highly compressible in nature.

Here, a substance when placed in a 100-mL square box have spherical shape and 50 mL volume. The shape and volume of the substance do not change when it is placed in a 100-mL circular tube, that means it does not change the shape with change of container and the state of substance will be solid.


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What is the [OH-] of a substance that has a pH of 11?
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How many coulombs are required to plate a layer of chromium metal 0.28 mm thick on an auto bumper with a total area of 0.40 m2 f
Rufina [12.5K]

Explanation:

The given data is as follows.

Thickness = 0.28 mm = 0.28 \times \frac{1}{10} cm = 0.028 cm

Area = 0.40 m^{2} = 0.40 \times 10^{4} cm^{2} = 4000 cm^{2}

As, it is known that volume = area × thickness

So,             Volume = 4000 cm^{2} \times 0.028 cm      

                                = 112 cm^{3}

As density is mass divided by volume. So, mass of chromium will be calculated as follows.

                   Density = \frac{mass}{volume}  

            7.20 g/cm^{3} = \frac{mass}{112 cm^{3}}      

                      mass = 806.4 g

As, mass of 1 mole of chromium is 52 g. So, number of moles in 806.4 g of chromium will be as follows.

              No. of moles = \frac{mass}{molar mass}                            

                                     = \frac{806.4 g}{52 g}

                                     = 15.50 mol

In chromate ion, (CrO^{2-}_{4}) charge on Cr is +6. It means that 6 electrons are needed to reduce Cr^{+6} into Cr.

As, 1 mole of Cr^{+6} ions require 6 moles of electrons. Therefore, moles of electrons for 15.50 mol will be calculated as follows.

                              6 × 15.50 mol = 93.04 mol

To calculate number of electrons we multiply number of moles by Avogadro's number as follows.

               93.04 mol \times 6.02 \times 10^{23}

                      = 560.13 \times 10^{23}

                     = 5.6 \times 10^{25} electrons

There is magnitude of 6.241 \times 10^{18} times the charge on an electron is equal to 1 coulomb.

Hence, number of coulombs will be as follows.

              No. of coulombs = \frac{5.6 \times 10^{25}}{6.241 \times 10^{18}}

                                           = 0.897 \times 10^{7} C

or,                                        = 8.97 \times 10^{6} C

Thus, we can conclude that 8.97 \times 10^{6} C are required to plate a layer of chromium metal with given data.

4 0
3 years ago
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