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3 years ago

Is one quarter the size of earth, has no moons, and has an almost non-existent atmosphere

Chemistry

2 answers:

natima [27]3 years ago

8 0

Answer:

MERCURY

Explanation:

PIT_PIT [208]3 years ago

7 0

For the answer to the question above,
If you mean planet, that would be Mercury. There are other objects in our solar system that could fit the criteria.
Our moon, Ganymede, and Callisto are about a quarter the size of Earth and have no atmosphere or moon.

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If a large marshmallow has a volume of 2.00 in3 and density of 0.242 g/cm3, how much would it weigh in grams? 1 in3=16.39 cm3.

siniylev [52]

First convert the inches cubed to centimeters cubed. Looking at the rate, we can write 2 inches cubed = 2 * 16.39 cm cubed = 32.78 cm cubed.

The equation for density is D = M/V, where D is the density, M is the mass, and V is the volume. Substitute the values into the equation:

0.242 = M/32.78

Multiply by 32.78 on both sides.

The mass is about 7.93 grams.

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4 years ago

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Lorico [155]

If the atom is neutral , the atomic number identifies the number of electrons in the atom.

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3 years ago

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Determine the mass in grams of 4.69 x 1021 atoms of barium. (The

Virty [35]

Answer:

1.07 g Ba

Explanation:

Hello there!

In this case, according to the definition of the Avogadro's number and the molar mass, it is possible to say that 6.022x10^{23} atoms of barium equal one mole, and at the same time, 1 mole equals 137.327 grams of this element; thus, it is possible to say that 6.022x10^{23} atoms of barium have a mass of 137.327 grams; therefore, it i possible for us to calculate the required mass in grams as shown below:

$4.69x10^{21}atoms*\frac{137.327gBa}{6.022x10^{23} atoms} \\\\=1.07gBa$

Best regards!

5 0

3 years ago

Determine the mass of 5.2 x 10 power of 21 molecules of propanol C3H7OH(l), on grams.

Alja [10]

$n(\text{C}_3\text{H}_7\text{OH}) = N(\text{C}_3\text{H}_7\text{OH}) / N_A\\ \phantom{n(\text{C}_3\text{H}_7\text{OH})} = 5.2 \times 10^{21} / (6.02 \times 10^{23})\\ \phantom{n(\text{C}_3\text{H}_7\text{OH})} = 8.6 \times 10^{-3} \; \text{mol}$

where $N_A = 6.02 \times 10^{23}\; \text{mol}^{-1}$ the Avogadro's constant that relates the number of particles to their number, in the unit moles $\text{mol}$ .

The molar mass of propanol- mass per mole propanol- can be directly deduced from its molecular formula with reference to a modern periodic table.

$M(\text{C}_3\text{H}_7\text{OH}) = \underbrace{3 \times 12.01}_{\text{carbon}} + \underbrace{8 \times 1.008}_{\text{hydrogen}} + \underbrace{1\times 16.00}_{\text{oxygen}} = 60.09 \; \text{g} \cdot \text{mol}^{-1}$

$8.6 \times 10^{-3} \; \text{mol}$ of propanol molecules would thus have a mass of $8.6 \times 10^{-3} \; \text{mol} \times 60.09 \; \text{g} \cdot \text{mol}^{-1} = 0.52 \; \text{g}$

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4 years ago

How many grams of al2br6 can be produced from 1278.4 g of br2 and 107.9g of al?

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3 years ago