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3 years ago

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Physics

1 answer:

Fed [463]3 years ago

6 0

please mark this answer as brainlist

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Analyze the effects on a passenger riding in a car traveling at

Mamont248 [21]

Without:

The passenger will get seriously injured
Colliding with the windshield at 50km/h
Could result in death

With safety:

The seatbelt holds tge passengers body back so they dont collide with anything
Their head is cushioned by the airbag
The passenger might get minor injuries but nothing serious will happen

5 0

2 years ago

marishachu [46]

Answer:

The box will experience an acceleration.

Explanation:

Here, 2 N and 3 N forces are acting opposite to each other. In this case, the net force experience by the box would be (3-2)N = 1 N towards right. Since acceleration is directly proportional to the net force, therefore the box will experience an acceleration.

6 0

3 years ago

4.6 billion years ago, the Earth is created from what

Musya8 [376]

Answer:

4.6 billion years ago the earth was made of gas and dust that was orbiting the newly forming Sun.

Explanation:

7 0

3 years ago

Problem Page Gaseous ethane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 28. g o

sergejj [24]

Answer : The maximum mass of carbon dioxide produced by the chemical reaction can be, 82.3 grams.

Solution : Given,

Mass of $C_2H_6$ = 28 g

Mass of $O_2$ = 190 g

Molar mass of $O_2$ = 32 g/mole

Molar mass of $C_2H_6$ = 30 g/mole

Molar mass of $CO_2$ = 44 g/mole

First we have to calculate the moles of $C_2H_6$ and $O_2$ .

$\text{ Moles of }C_2H_6=\frac{\text{ Mass of }C_2H_6}{\text{ Molar mass of }C_2H_6}=\frac{28g}{30g/mole}=0.933moles$

$\text{ Moles of }O_2=\frac{\text{ Mass of }O_2}{\text{ Molar mass of }O_2}=\frac{190g}{32g/mole}=5.94moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

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

From the balanced reaction we conclude that

As, 2 mole of $C_2H_6$ react with 7 mole of $O_2$

So, 0.933 moles of $C_2H_6$ react with $\frac{7}{2}\times 0.933=3.26$ moles of $O_2$

From this we conclude that, $O_2$ is an excess reagent because the given moles are greater than the required moles and $C_2H_6$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $CO_2$

From the reaction, we conclude that

As, 2 mole of $C_2H_6$ react to give 4 mole of $CO_2$

So, 0.933 moles of $C_2H_6$ react to give $\frac{4}{2}\times 0.933=1.87$ moles of $CO_2$