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tekilochka [14]
2 years ago
9

The heat from the bonfire is transferred to the student's hands through the process of

Chemistry
1 answer:
Agata [3.3K]2 years ago
3 0

Answer:

Radiation

Explanation:

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There would be 79 electrons present in each atom of gold. I hope this helps :)
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In which region is the substance in both the solid phase and the liquid phase ?
sergiy2304 [10]

Answer:  Region 3

Explanation:  The temperature and time graph suggests that region 3 is the region in which the substance can co exist in both the phases that is solid phase and liquid phase.

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Read 2 more answers
Gaseous ethane (CH,CH,) will react with gaseous oxygen (02) to produce gaseous carbon dioxide (CO2) and gaseous water (H,0). Sup
BigorU [14]

<u>Answer:</u> The mass of CO_2 produced is 12.32 g

<u>Explanation:</u>

The number of moles is defined as the ratio of the mass of a substance to its molar mass.  The equation used is:

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

  • <u>For ethane:</u>

Given mass of ethane = 4.21 g

Molar mass of ethane = 30 g/mol

Putting values in equation 1, we get:

\text{Moles of ethane}=\frac{4.21g}{30g/mol}=0.140mol

  • <u>For oxygen gas:</u>

Given mass of oxygen gas = 31.9 g

Molar mass of oxygen gas= 32 g/mol

Putting values in equation 1, we get:

\text{Moles of oxygen gas}=\frac{31.9g}{32g/mol}=0.997mol

The chemical equation for the combustion of ethane follows:

2C_2H_6+7O_2\rightarrow 4CO_2+6H_2O

By stoichiometry of the reaction:

If 2 moles of ethane reacts with 7 moles of oxygen gas  

So, 0.140 moles of ethane will react with = \frac{7}{2}\times 0.140=0.49mol of oxygen gas

As the given amount of oxygen gas is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.

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

By the stoichiometry of the reaction:

If 2 moles of ethane produces 4 moles of CO_2

So, 0.140 moles of ethane will produce = \frac{4}{2}\times 0.140=0.28mol of CO_2

We know, molar mass of CO_2 = 44 g/mol

Putting values in above equation, we get:

\text{Mass of }CO_2=(0.28mol\times 44g/mol)=12.32g

Hence, the mass of CO_2 produced is 12.32 g

7 0
2 years ago
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