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2 years ago

8

Which of the following atoms would bond covalently? A. Silicon and sulfur B. Carbon and neon C. Lithium and fluorine D. Calcium

and magnesium

1 answer:

lord [1]2 years ago

3 0

Answer:

For example water is a covalent compound which is formed by the covalent bonding between hydrogen and oxygen atom.

Explanation:

You might be interested in

Find the amount in kJ of heat exchanged by the combustion of 61.9 g of ethane (C2H6(8) given that the molar enthalpy of combusti

elena-14-01-66 [18.8K]

Answer:

2994 kJ

Explanation:

When one mol of ethane (C₂H₆) is combusted, 1451 kJ of heat is exchanged.

First we convert 61.9 g of C₂H₆ into moles, using its molar mass:

61.9 g ÷ 30 g/mol = 2.06 mol C₂H₆

Finally we <u>calculate how much heat is exchanged by the combustion of 2.06 moles of C₂H₆</u>:

2.06 mol * 1451 kJ/mol = 2994 kJ

8 0

2 years ago

Which structure of the cell controls what goes in and comes out of the cell?

LenKa [72]

The Cell Membrane.

The Cell Membrane wraps around the entire cell and only allows certain things to pass through, blocking out potentially harmful things from the organelles within the cell.

Hope this helps!

7 0

2 years ago

Part B When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 22.8 g of carbon were burned in the pres

aksik [14]

<u>Answer:</u> The amount of carbon dioxide gas produced in the reaction is 83.6 grams

<u>Explanation:</u>

As, some amount of oxygen gas is left after the reaction is completed. So, it is present in excess and is considered as an excess reagent.

Thus, carbon is considered as a limiting reagent because it limits the formation of product.

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of carbon = 22.8 g

Molar mass of carbon = 12 g/mol

Putting values in equation 1, we get:

$\text{Moles of carbon}=\frac{22.8g}{12g/mol}=1.9mol$

The chemical equation for the reaction of carbon and oxygen gas follows:

$C+O_2\rightarrow CO_2$

By Stoichiometry of the reaction:

1 mole of carbon produces 1 mole of carbon dioxide gas

So, 1.9 moles of carbon will produce = $\frac{1}{1}\times 1.9=1.9moles$ of carbon dioxide gas

Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 1.9 moles

Putting values in equation 1, we get:

$1.9mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(1.9mol\times 44g/mol)=83.6g$

Hence, the amount of carbon dioxide gas produced in the reaction is 83.6 grams

6 0

2 years ago

Upper n subscript 2 (g) plus 3 upper H subscript 2 (g) double-headed arrow 2 upper N upper H subscript 3 (g). At equilibrium, th

artcher [175]

Answer:

The <u>equilibrium constant</u> is:

$k_c=0.0030M^{-2}$

Explanation:

The correct equation is:

N₂(g) + 3H₂(g) ⇄ 2NH₃(g)

Thus, with the equilibrium concentrations you can calculate the equilibrium constant, Kc.

The equation for the equilibrium constant is:

$k_c=\dfrac{[NH_3]^2}{[N_2]\cdot [H_2]^3}$

Substituting:

$k_c=\dfrac{(0.105M)^2}{(1.1M)\cdot (1.50M)^3}$

$k_c=0.0030M^{-2}$

6 0

3 years ago

How much energy is used to heat 250 g of ice from –15°C to steam at 105°C? (Hint: 5 steps, all positive)

lianna [129]

Answer:

Explanation: Q1 = mc(ice) ΔT (ice warms)

Q2 = ms (ice melts)

Q3 = mc((water) ΔT (water warms)

Q4 = mr (water boils)

Q5 = mc(vapour)ΔT

7 0

2 years ago