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prohojiy [21]
2 years ago
12

Hypothesis: If a fixed amount of gas is heated,

Chemistry
2 answers:
dezoksy [38]2 years ago
6 0

Answer:

If fixed amount of gas is heated then the volume will increase because the heat will cause the molecules of gas to move freely and increase the kinetic energy.

Explanation:

If fixed amount of gas is heated then the volume will increase because the heat will cause the molecules of gas to move freely and increase the kinetic energy.

According to the Charle's law

The volume of given amount of gas is directly proportional to the temperature at constant pressure and number of moles of gas.

Mathematical expression;

V ∝ T

V = kT

V/T = k

if volume is changed from V1 to V2 and temperature change from T1 to T2 then,

V1/T1 = k      V2/T2= k

V1/T1 = V2/T2

Reptile [31]2 years ago
6 0

Increase

faster and further apart.

Explanation: I just took it.

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A transition in the balmer series for hydrogen has an observed wavelength of 434 nm. Use the Rydberg equation below to find the
DanielleElmas [232]

Answer:

i. n = 5

ii. ΔE = 7.61 × 10^{-46} KJ/mole

Explanation:

1. ΔE = (1/λ) = -2.178 × 10^{-18}(\frac{1}{n^{2}_{final} } - \frac{1}{n^{2}_{initial}  })

    (1/434 × 10^{-9}) = -2.178 × 10^{-18} (\frac{n^{2}_{initial} - n^{2}_{final}  }{n^{2}_{final} n^{2}_{initial}   })

⇒ 434 × 10^{-9} = (1/-2.178 × 10^{-18})\frac{n^{2}_{final} *n^{2}_{initial}   }{n^{2}_{initial} - n^{2}_{final}    }

But, n_{final} = 2

434 × 10^{-9} = (1/2.178 × 10^{-18})\frac{2^{2} n^{2}_{initial}  }{n^{2}_{initial} - 2^{2}  }

434 × 10^{-9}  × 2.178 × 10^{-18} = (\frac{4n^{2}_{initial}  }{n^{2}_{initial} - 4 })

⇒ n_{initial} = 5

Therefore, the initial energy level where transition occurred is from 5.

2. ΔE = hf

     = (hc) ÷ λ

    = (6.626 × 10−34 × 3.0 × 10^{8} ) ÷ (434 × 10^{-9})

    = (1.9878 × 10^{-25}) ÷ (434 × 10^{-9})

    = 4.58 × 10^{-19} J

    = 4.58 × 10^{-22} KJ

But 1 mole = 6.02×10^{23}, then;

energy in KJ/mole = (4.58 × 10^{-22} KJ) ÷ (6.02×10^{23})

         = 7.61 × 10^{-46} KJ/mole

7 0
2 years ago
How many liters of radon gas would be in 3.43 moles at room temperature and pressure (293 K and 100 kPa)?
OLga [1]

Using ideal gas equation,

P\times V=n\times R\times T

Here,

P denotes pressure

V denotes volume

n denotes number of moles of gas

R denotes gas constant

T denotes temperature

The values at STP will be:

P=100 kPa

T=293 K

R=8.314472 L kPa K⁻¹ mol⁻¹

Number of moles of gas=3.43 mole

Putting all the values in the above equation,

V=\frac{3.43\times 8.314\times 293}{100}

V=83.55 L

So the volume will be 83.55 L.

83.55 L of radon gas would be in 3.43 moles at room temperature and pressure (293 K and 100 kPa).

4 0
2 years ago
Stars, such as our sun, use fusion to combine hydrogen atoms into helium atoms, and in the process, create energy. As massive st
Zinaida [17]

Hey there! The answer to your first question is SILICON, Nickle has 28 protons, silicon has 14, 14+14=28. Its the only element thats adds up. I dont know about the 2nd one myself.

4 0
2 years ago
How many paired and unpaired electrons are in magnesium?
pychu [463]

Answer:

Paired = 12

Unpaired = 0

Explanation:

Magnesium is alkaline earth metal.

It is present in second group.

Its atomic number is 12 and atomic mass 24 amu.

Electronic configuration:

Mg₁₂ = 1s² 2s² 2p⁶ 3s²

It can seen from electronic configuration that all electrons are paired because s subshell have one orbital and it can accomodate two electrons. Each s subshells in magnesium have two electrons so these are filled and have paired electrons. While p subshell have three orbitals and can accomodate six electrons two by each orbital with opposite spin thus 2p is also filled and have paired electrons.

8 0
2 years ago
Calculate the mass of silver nitrate (in grams) in a 145 mL solution of 5.88 M AgNO3?
oee [108]
1 mole of AGNO3 weighs 170g
so 0.6322 miles will weigh 170 X 0.6322=107.474 g
6 0
2 years ago
Read 2 more answers
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