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Pachacha [2.7K]
3 years ago
15

What is the velocity of a skateboarder whose momentum is 100 kg-m/s and mass is 15 kg? Round to the nearest hundredth. A. 3.33 m

/s B. 13.25 m/s C. 6.67 kg D. 6.67 m/s
Chemistry
2 answers:
Serjik [45]3 years ago
7 0

Answer: D

Explanation: 100/15 =6.67 I hope this is right.

Inessa [10]3 years ago
4 0

Answer : The correct option is, (D) 6.67 m/s

Explanation : Given,

Momentum = 100 Kg m/s

Mass = 15 Kg

Momentum : It is defined a the product of mass and the velocity of an object.

Formula used :

p=mv

where,

p = momentum

m = mass

v = velocity

Now put all the given values in the above formula, we get the velocity of a skateboarder.

100\text{Kg m/s}=15Kg\times v

v=6.67m/s

Therefore, the velocity of a skateboarder is, 6.67 m/s

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Answer :

The mass of excess mass of Na_2CO_3, AgNO_3,Ag_2CO_3\text{ and }NaNO_3 are, 1.908 g, 0 g, 12.144 g and 3.74 g respectively.

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Mass of Na_2CO_3 = 4.25 g

Mass of AgNO_3 = 7.50 g

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Molar mass of AgNO_3 = 170 g/mole

Molar mass of Ag_2CO_3 = 276 g/mole

Molar mass of NaNO_3 = 85 g/mole

First we have to calculate the moles of Na_2CO_3 and AgNO_3.

\text{Moles of }Na_2CO_3=\frac{\text{Mass of }Na_2CO_3}{\text{Molar mass of }Na_2CO_3}=\frac{4.25g}{106g/mole}=0.040moles

\text{Moles of }AgNO_3=\frac{\text{Mass of }AgNO_3}{\text{Molar mass of }AgNO_3}=\frac{7.50g}{170g/mole}=0.044moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

Na_2CO_3+2AgNO_3\rightarrow Ag_2CO_3+2NaNO_3

From the balanced reaction we conclude that

As, 2 moles of AgNO_3 react with 1 mole of Na_2CO_3

So, 0.044 moles of AgNO_3 react with \frac{0.044}{2}=0.022 moles of Na_2CO_3

From this we conclude that, Na_2CO_3 is an excess reagent because the given moles are greater than the required moles and AgNO_3 is a limiting reagent and it limits the formation of product.

The excess mole of Na_2CO_3 = 0.040 - 0.022 = 0.018 mole

Now we have to calculate the mass of excess mole of Na_2CO_3.

\text{Mass of }Na_2CO_3=\text{Moles of }Na_2CO_3\times \text{Molar mass of }Na_2CO_3=(0.018mole)\times (106g/mole)=1.908g

Now we have to calculate the moles of Ag_2CO_3.

As, 1 moles of AgNO_3 react to give 1 moles of Ag_2CO_3

So, 0.044 moles of AgNO_3 react to give 0.044 moles of Ag_2CO_3

Now we have to calculate the mass of AgCO_3.

\text{Mass of }Ag_2CO_3=\text{Moles of }Ag_2CO_3\times \text{Molar mass of }Ag_2CO_3=(0.044mole)\times (276g/mole)=12.144g

Now we have to calculate the moles of NaNO_3.

As, 2 moles of AgNO_3 react to give 2 moles of NaNO_3

So, 0.044 moles of AgNO_3 react to give 0.044 moles of NaNO_3

Now we have to calculate the mass of NaNO_3.

\text{Mass of }NaNO_3=\text{Moles of }NaNO_3\times \text{Molar mass of }NaNO_3=(0.044mole)\times (85g/mole)=3.74g

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