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rusak2 [61]
3 years ago
14

Which characteristic of a planet describes whether the planet has a thick or thin layer of gas?

Chemistry
2 answers:
raketka [301]3 years ago
8 0
Atmosphere I took the test
Inessa [10]3 years ago
3 0

Answer:

Atmoshphere!

Explanation:

I took the test and got a 100%! :) Hope this helps, plz mark brainliest!

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An increase in pressure increasing the boiling point of a liquid is an example of a —
Setler [38]

Answer:

Ans. C. physical change

Explanation:

Physical: boiling and melting are physical changes. When water boils no bonds are broken or formed

5 0
3 years ago
An aqueous 0.300 M glucose solution is prepared with a total volume of 0.150 L. The molecular weight of
Rudik [331]

Answer:

8.11g

Explanation:

Given parameters:

Molarity of aqueous solution = 0.3M

total volume  = 0.15L

Molecular weight of glucose  = 180.6g/mol

Unknown:

Mass of glucose needed in the solution = ?

Solution:

To solve this problem, we need to understand molarity.

Molarity is the number of moles of solute in a given volume of solution. In this problem, the solute here is the glucose and the solvent is water.

      Molarity  = \frac{number of moles of solute}{volume of solution}

A solution is made up of solute and solvent.

   now, let us solve for the number of moles of the solute which is glucose;

   Number of moles of glucose  = molarity x volume of solution;

                                                      = 0.3 x 0.15

                                                      = 0.045mole

Now to find the mass of glucose;

        mass of glucose  = number of moles x molar mass

             input the parameters;

       

         Mass of glucose  = 0.045  x 180.16 = 8.11g

4 0
3 years ago
How many grams of H2 can be formed from 54.6 grams of NH3 in the following reaction? 2NH3 (g) --> 3H2 (g) + N2 (g)
Strike441 [17]

Answer:

9.64g

Explanation:

The balanced equation for the reaction is given below:

2NH3 (g) —> 3H2 (g) + N2 (g)

Next, we need to calculate the mass NH3 that decomposed and the mass of H2 produced from the balanced equation. This is illustrated below:

Molar Mass of NH3 = 14 + (3x1) = 14 + 3 = 17g/mol

Mass of NH3 that decomposed from the balanced equation = 2 x 17 = 34g

Molar Mass of H2 = 2x1 = 2g/mol

Mass of H2 produced from the balanced equation = 3 x 2 = 6g.

Now, we can obtain the mass of H2 formed from 54.6g of NH3 as follow:

From the balanced equation above,

34g of NH3 decomposed to produce 6g of H2.

Therefore, 54.6g of NH3 will decompose to produce = (54.6x6)/34 = 9.64g of H2

Therefore, 9.64g of H2 can be obtained from 54.6g of NH3.

3 0
3 years ago
Assessment started: undefined.
AveGali [126]

Answer:

(C) knowing which minerals are in a rock can help you identify and classify that rock.

Explanation:

It is the truth.

8 0
4 years ago
At 1000 K the Kc value for the following reaction is 1.5 × 10⁶ (1) N₂O₄ (g) ⇌ 2 NO₂ (g) At 1000 K the Kc value for the following
Ahat [919]

Answer:

The value of Kc is 9.33 * 10^-17

Explanation:

Step 1: Data given

Temperature = 1000 K

N₂O₄ (g) ⇌ 2 NO₂ (g) Kc = 1.5 * 10^6

N₂ (g) + 2 O₂(g) ⇌ 2 NO₂ (g)  Kc = 1.4 * 10^-10

Step 2: Calculate Kc for  N₂ (g) + 2 O₂ ⇌ N₂O₄

N₂O₄ (g) ⇌ 2 NO₂ (g) Kc = 1.5 * 10^6

2 NO₂ (g) ⇌  N₂O₄ (g)    = 1/Kc = 1 / 1.5 * 10^6   = 6.67 *10^-7

N₂ (g) + 2 O₂(g) ⇌ 2 NO₂ (g)  Kc = 1.4 * 10^-10

Kc = Kc1 * Kc2

Kc = (6.67 *10^-7) * (1.4 * 10^-10)

Kc = 9.33 * 10 ^-17

The value of Kc is 9.33 * 10^-17

4 0
3 years ago
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