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3 years ago

Which of the following is most likely to dissolve in NH3? A) CO2 B) CH4 C) H2S D) BH3

Chemistry

1 answer:

dem82 [27]3 years ago

5 0

Answer:

C) H2S

Explanation:

In chemistry, the dissolution of one substance in another is dependent on the magnitude of intermolecular interaction between the two substances. Hence, if two substances do not interact in one way or the other, then one can not dissolve the other.

Let us consider the fact that NH3 is a polar molecule and it is a general principle that like dissolves like. Hence, only H2S which is also a polar molecule can effectively interact with NH3 due to dipole-dipole interaction between the two molecules.

Also, ammonia reacts with hydrogen sulphide as follows;

2NH3 + H2S → (NH4)2S

Hence H2S is more likely to dissolve in NH3.

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How many moles are in 6.80 x 10^23 atoms of gold, Au?

frosja888 [35]

Answer:

1.13 moles Au

Explanation:

Moles Au = 6.80x10²³atoms / 6.023x10²³atoms/mole = 1.13 moles Au

8 0

2 years ago

The volume of a Goodyear Blimp is 2.5x10^7 L, which is occupied by 1.7x10^6 mol of helium. What is the internal pressure of the

attashe74 [19]

Answer:

1.7 bar

Explanation:

We can use the Ideal Gas Law to calculate the individual gas pressure.

pV = nRT Divide both sides by V

p = (nRT)/V

Data: n = 1.7 × 10⁶ mol

R = 0.083 14 bar·L·K⁻¹mol⁻¹

T = 22 °C

V = 2.5 × 10⁷ L

Calculations:

(a) Change the temperature to kelvins

T = (22 + 273.15) K

= 295.15 K

(b) Calculate the pressure

p = (1.7 × 10⁶ × 0.083 14 × 295.15)/(2.5× 10⁷)

= 1.7 bar

4 0

3 years ago

The oxidation numbers of nitrogen in nh3, hno3, and no2 are, respectively:

vovikov84 [41]

The oxidation numbers for Nitrogen are respectively -3, +5, +4

3 0

3 years ago

Read 2 more answers

If 16.00 g of O₂ reacts with 80.00 g NO, how many the excess reactant are left over? (enter only the value, round to whole numbe

pishuonlain [190]

Answer:

Explanation:

We will need a balanced equation with masses, moles, and molar masses of the compounds involved.

1. Gather all the information in one place with molar masses above the formulas and masses below them.

Mᵣ: 30.01 32.00 46.01

2NO + O₂ ⟶ 2NO₂

Mass/g: 80.00 16.00

2. Calculate the moles of each reactant

$\text{moles of NO} = \text{80.00 g NO} \times \dfrac{\text{1 mol NO}}{\text{30.01 g NO}} = \text{2.666 mol NO}\\\\\text{moles of O}_{2} = \text{16.00 g O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{32.00 g O}_{2}} = \text{0.5000 mol O}_{2}$