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pychu [463]
3 years ago
10

- How much power does it take to lift a 1,000 N load 10 m in 20 s?

Chemistry
1 answer:
Mariana [72]3 years ago
5 0

Answer:

"500 Joule/sec" is the right answer.

Explanation:

The given values are:

Force,

F = 1000 N

Velocity,

s = 10 m

Time,

t = 20 s

Now,

The power will be:

=  \frac{Force\times Velocity}{Time}

On putting the values, we get

=  \frac{1000\times 10}{20}

=  \frac{10000}{20}

=  500 \ Joule/sec

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One liter of air contains about 0.21 L of oxygen. When filled, the human lungs hold about 6.0 L of air. How much oxygen is in th
masya89 [10]
Since we are told that 1L of air contains 0.21L of oxygen, you can use the conversion (0.21L O₂)/(1L air).  That means that you can just multiply 6.0L by 0.21L to get 1.26L of O₂.
that means that the lungs can hold about 1.26L of oxygen.
I hope this helps.  Let me know if anything is unclear.
4 0
3 years ago
How many moles of O atoms are present in a 254 g sample of carbon dioxide?
MaRussiya [10]

Answer:

11.6mol

Explanation:

CO2 = 44g

2 mol of O2 = 44g

X mol of O2 = 254

Cross multiply

X= 11.6mol

3 0
2 years ago
2.0L of hydrogen gas is mixed with 3.0L of nitrogen gas at STP in a rigid 5.0L vessel. A reaction occurs, producing ammonia gas
IrinaK [193]

Answer:

Moles NH₃: 0.0593

0.104 moles of N₂ remain

Final pressure: 0.163atm

Explanation:

The reaction of nitrogen with hydrogen to produce ammonia is:

N₂ + 3 H₂ → 2 NH₃

Using PV = nRT, moles of N₂ and H₂ are:

N₂: 1atmₓ3.0L / 0.082atmL/molKₓ273K = 0.134 moles of N₂

H₂: 1atmₓ2.0L / 0.082atmL/molKₓ273K = 0.089 moles of H₂

The complete reaction of N₂ requires:

0.134 moles of N₂ × (3 moles H₂ / 1 mole N₂) = <em>0.402 moles H₂</em>

That means limiting reactant is H₂. And moles of NH₃ produced are:

0.089 moles of H₂ × (2 moles NH₃ / 3 mole H₂) = <em>0.0593 moles NH₃</em>

Moles of N₂ remain are:

0.134 moles of N₂ - (0.089 moles of H₂ × (1 moles N₂ / 3 mole H₂)) = <em>0.104 moles of N₂</em>

And final pressure is:

P = nRT / V

P = (0.104mol + 0.0593mol)×0.082atmL/molK×273K / 5.0L

<em>P = 0.163atm</em>

7 0
3 years ago
In boyle's law, the initial volume of a gas is 120 ml at 256 kpa. what will be the volume if the pressure increases to 385 kpa?
Vinil7 [7]
<h3>Answer:</h3>

79.8 ml

<h3>Explanation:</h3>

Boyle's law describes the relationship between pressure and volume when the temperature is constant. For this question, I will be rounding to significant figures.

Boyle's Formula

When describing the relationship between pressure and volume, the formula \displaystyle P_{1} V_{1}= P_{2} V_{2}. In this formula, P_{1}V_{1} is the initial pressure and volume. On the other side, P_{2} V_{2} is final pressure and volume. So, to find a missing variable you must plug in the values you are given.

Final Volume

Remember when solving this question to remain constant in your units. When we plug in the values we know we are given:

  • 256kPa*120mL=385kPa*V_{2} mL

Now, we can multiply the left side

  • 30720kPa*mL=385kPa*V_{2} mL

Finally, we can divide by 385 to isolate the final volume

  • 79.8mL=V_{2}

This gives the final volume of 79.8mL.

7 0
2 years ago
Which of the following statements is true?
Kazeer [188]
Only one: the nucleus of an atom is made up of protons and neutrons.
Why others are false:
Boiling point of a substance is not dependent on the volume because it’s a intensive property.
During sublimation, a solid changes directly into gas.
Electrons orbit the nucleus of an atom in circular orbits (kinda unsure of this one.)
3 0
3 years ago
Read 2 more answers
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