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kramer
3 years ago
6

how much hydrogen gas is necessary to exert a pressure of 1.4 ATM at 430k if occupying a volume of 15.1 l

Chemistry
1 answer:
lora16 [44]3 years ago
7 0

Answer:

5

Explanation:

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15 pts The drop down items have the same options for all sections labeled choose an item
cricket20 [7]

8) 21.504 liters of gas

9) 122.5 g

10) 6.022*10^23

Explanation:

8)

1 mole= 22.4 liters

to calculate the volume of gas of 0.960 moles of CH4

22.4*0.960/1

= 21.504 liters of gas  

9)

2.0 mole*18.02 g/ 1 mole

=122.5 g

10)

2.0 l * 1 mole/22.4 l

6.022*10^23

8 0
3 years ago
The molar mass of an element is the mass of one
allochka39001 [22]

Answer:

  • <em>The molar mass of an element is the mass of </em><u>one mole of atoms of the element.</u>

Explanation:

<em>The molar mass of an element </em>is its atomic mass, i.e.  the mass in grams of one mole of atoms of the element.

Remember 1 mol is approximately 6.022 × 10²³.

So, 1 mol of atoms is 6.022 × 10²³ atoms.

The molar mass is an average: it is the weighted average mass of the natural isotopes of the element, taking into account their relative abundance.

For example, the molar mass or atomic mass of carbon is 12,0107 g/mol, instead of 12.0000, becasue carbon exists in several forms (isotopes), and so the weighted average is not a whole number.

7 0
3 years ago
A person uses a pulley to raise a flag up a 15 meter flagpole. The weight of
GREYUIT [131]

Answer:

Explanation:

I burnt my ramen noodles today :) <3 help me <3 I need somewhere to live

8 0
3 years ago
*multiple choice*
galben [10]

1.95  or 2  is the molarity of a 45.3g sample of KNO3 (101g) dissolved in enough water to make a 0.225L solution.

The correct answer is option b

Explanation:

Data given:

mass of KNO_{3} = 45.3 grams

volume = 0.225 litre

molarity =?

atomic mass of KNO3 = 101 grams/mole

molarity is calculated by using the formula:

molarity = \frac{number of moles}{volume of the solution}

first the number of moles present in the given mass is calculated as:

number of moles = \frac{mass}{atomic mass of 1 mole}

number of moles = \frac{45.3}{101}

0.44 moles of KNO3

Putting the values in the equation of molarity:

molarity = \frac{0.44}{0.225}

molarity = 1.95

It can be taken as 2.

The molarity of the potassium nitrate solution is 2.

7 0
2 years ago
Need help on last 3 questions
Olin [163]

Answer:

Explanation:

1)

Given data:

Initial volume of balloon = 0.8 L

Initial temperature = 12°C ( 12+273= 285 K)

Final temperature = 300°C (300+273 = 573 K)

Final volume = ?

Solution:

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁  

V₂ = 0.8 L .573 K / 285 K

V₂ = 458.4 L / 285

V₂ = 1.61 L

2)

Initial pressure = 204 kpa

Initial temperature = 29°C ( 29 + 273 = 302 K)

Final temperature = ?

Final pressure = 300 kpa

Solution:

P₁/T₁ = P₂/T₂

T₂ = T₁P₂/P₁  

T₂ = 302 K . 300 kpa / 204 kpa

T₂ = 90600 K/ 204

T₂ = 444.12 K

3)

Given data:

Initial volume = 14 L

Initial pressure = 2.1 atm

Initial temperature = 100 K

Final temperature = 450 K

Final volume = ?

Final pressure = 1.2 atm

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 2.1 atm × 14 L × 450 K / 100 K × 1.2 atm  

V₂ = 13230 L / 120

V₂ = 110.25 L

5 0
3 years ago
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