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Varvara68 [4.7K]
3 years ago
14

If I have 1.9 moles of gas held at a pressure of 5 atm and in a container with a

Chemistry
1 answer:
ohaa [14]3 years ago
6 0

Explanation:

gas has a temperature of 100C at a pressure of 105atm. What is the temperature at 50 atm?

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What are the steps of natural selection?
blagie [28]

Answer:

The five steps involved in the process of natural selection are

Variation • Inheritance • Selection • Time • Adaptation

☆anvipatel77☆

•Expert•

Brainly Community Contributor

5 0
2 years ago
The rate of effusion of an unknown gas was measured and found to be 11.9 mL/min. Under identical conditions, the rate of effusio
iren2701 [21]

Answer : The correct option is, (B) CO_2

Solution :

According to the Graham's law, the rate of effusion of gas is inversely proportional to the square root of the molar mass of gas.

R\propto \sqrt{\frac{1}{M}}

or,

(\frac{R_1}{R_2})=\sqrt{\frac{M_2}{M_1}}       ..........(1)

where,

R_1 = rate of effusion of unknown gas = 11.9\text{ mL }min^{-1}

R_2 = rate of effusion of oxygen gas = 14.0\text{ mL }min^{-1}

M_1 = molar mass of unknown gas  = ?

M_2 = molar mass of oxygen gas = 32 g/mole

Now put all the given values in the above formula 1, we get:

(\frac{11.9\text{ mL }min^{-1}}{14.0\text{ mL }min^{-1}})=\sqrt{\frac{32g/mole}{M_1}}

M_1=44.2g/mole

The unknown gas could be carbon dioxide (CO_2) that has approximately 44 g/mole of molar mass.

Thus, the unknown gas could be carbon dioxide (CO_2)

5 0
3 years ago
Help with this question please i will mark you brainliest!!!
tamaranim1 [39]

Answer:

b

Explanation:

5 0
3 years ago
Read 2 more answers
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makkiz [27]
Climate change is likely causing parts of the water cycle to speed up as warming global temperatures increase the rate of evaporation worldwide. More evaporation is causing more precipitation, on average.
May God bless you and your family
7 0
3 years ago
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation
zysi [14]
Hope it helped you.

7 0
4 years ago
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