2 years ago

Which type of bond will form between these elements? *

Chemistry

1 answer:

BlackZzzverrR [31]2 years ago

6 0

Answer:

Please mention elements so i can answer it

Explanation:

You might be interested in

Examples of light effecting chemical change

Annette [7]

Answer:

burning of wood ,cooking an egg,baking a cake,rusting of iron,digestion of food .

8 0

2 years ago

La masa molar para el siguiente compuesto: CuOH, si sus masas atómicas son Cu=64 g/mol; O=16 g/mo e H=1 g/mol

aev [14]

Answer:

Abraham Lincoln

..,,,,,

4 0

2 years ago

Read 2 more answers

To test the effectiveness of a gunpowder mixture, 1 gram was exploded under controlled STP conditions, and the reaction chamber

Alekssandra [29.7K]

Answer:

1.3 × 10³ cm³

Explanation:

The gas occupies a volume of V₁ = 310 cm³ under standard temperature and pressure (STP), that is, T₁ = 273.15 K and P₁ = 1.0 atm. In order to find the volume V₂ under different conditions we can use the combined gas law formula.

$\frac{P_{1}.V_{1}}{T_{1}} =\frac{P_{2}.V_{2}}{T_{2}} \\V_{2}=\frac{P_{1}.V_{1}.T_{2}}{T_{1}.P_{2}}=\frac{1.0atm\times 310cm^{3} \times 2473K }{273.15K \times 2.1atm} =1.3 \times 10^{3} cm^{3}$

7 0

2 years ago

How many valence electrons are in atom of sulfur?

Nookie1986 [14]

The answer is six because it is in group six A on the periodic table.

8 0

2 years ago

You are the medical examiner at the scene of a murder at a restaurant. There is a

Hoochie [10]

The compound : C₄₀H₄₄N₄O

<h3>Further explanation</h3>

The empirical formula is the smallest comparison of atoms of compound =mole ratio of the components

The principle of determining empirical formula

• Determine the mass ratio of the constituent elements of the compound.

• Determine the mole ratio by dividing the percentage by the atomic mass

The mol ratio of composition : C : H : N : O

$\tt \dfrac{80.66}{12}\div \dfrac{7.39}{1}\div \dfrac{9.39}{14}\div \dfrac{2.68}{16}\\\\6.722\div 7.39\div 0.671\div 0.1675\rightarrow divide~by~smallest(0.1675)\\\\40\div 44\div 4\div 1$

3 0

2 years ago