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andre [41]
3 years ago
8

1. If you have 5g of pennies how many dozen pennies do you have?

Chemistry
1 answer:
likoan [24]3 years ago
4 0

Answer:

15.69 dozen

Explanation:

Mass of penny = 5 g

Dozens of penny =..?

Next, we shall convert 5 g to gross. This can be obtained as follow:

3824 g = 1000 gross

Therefore,

5 g = 5 g × 1000 gross / 3824 g

5 g = 1.3075 gross

Thus, 5 g is equivalent to 1.3075 gross.

Finally, we convert 1.3075 gross to dozen. This can be obtained as follow:

1 gross = 12 dozen

Therefore,

1.3075 gross = 1.3075 gross × 12 dozen / 1 gross

1.3075 gross = 15.69 dozen

Thus, 5 g of penny is equivalent to 15.69 dozen

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3 years ago
John rode 3150 m at an average speed of 350 m/min.If he had ridden at average of 375 m/min instead. How much sooner would it hav
Svet_ta [14]

Explanation:

Given that:

Distance traveled = 3150m

Average speed = 350m/min

Suggested speed = 375m/min

Unknown:

Time = ?

Solution:

Speed is the rate of change of distance with time.

  it is mathematically expressed as;

     speed = \frac{distance }{time}

Initial time using speed 350m/min can be calculated by making time the subject of the formula;

     time taken = \frac{distance }{speed}

    time taken at speed of speed of 350m/min = \frac{3150}{350} = 9min

   to seconds = 9 x 60 = 540 seconds

  time taken at speed of 375m/min = \frac{3150}{375} = 8.4min

   to seconds = 8.4 x 60 = 504 seconds.

It could have taken 504 seconds sooner saving 36 seconds.

learn more:

Speed brainly.com/question/10177389

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7 0
3 years ago
First person with the right answer gets brainliest thanks (btw the numbers on the right are the answers choose the right one)
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3 years ago
Nitrogen gas reacts with hydrogen gas to produce ammonia. How many liters of hydrogen gas at 95kPa and 15∘C are required to prod
viktelen [127]

Answer:

222.30 L

Explanation:

We'll begin by calculating the number of mole in 100 g of ammonia (NH₃). This can be obtained as follow:

Mass of NH₃ = 100 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3

= 17 g/mol

Mole of NH₃ =?

Mole = mass /molar mass

Mole of NH₃ = 100 / 17

Mole of NH₃ = 5.88 moles

Next, we shall determine the number of mole of Hydrogen needed to produce 5.88 moles of NH₃. This can be obtained as follow:

N₂ + 3H₂ —> 2NH₃

From the balanced equation above,

3 moles of H₂ reacted to produce 2 moles NH₃.

Therefore, Xmol of H₂ is required to p 5.88 moles of NH₃ i.e

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Finally, we shall determine the volume (in litre) of Hydrogen needed to produce 100 g (i.e 5.88 moles) of NH₃. This can be obtained as follow:

Pressure (P) = 95 KPa

Temperature (T) = 15 °C = 15 + 273 = 288 K

Number of mole of H₂ (n) = 8.82 moles

Gas constant (R) = 8.314 KPa.L/Kmol

Volume (V) =?

PV = nRT

95 × V = 8.82 × 8.314 × 288

95 × V = 21118.89024

Divide both side by 95

V = 21118.89024 / 95

V = 222.30 L

Thus the volume of Hydrogen needed for the reaction is 222.30 L

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</span>[H⁺] = 10∧-pH.
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