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uranmaximum [27]
2 years ago
11

What happens when an electron moves from n=2 to n=5?

Chemistry
1 answer:
Aleksandr-060686 [28]2 years ago
4 0

Answer:

Explanation:

10?

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Calculate the change in entropy if Br2(l) is converted to Br2(g).
Alik [6]

Ans: The entropy change for the given reaction is 93.3 J/K

Given reaction:

Br2(l) → Br2(g)

ΔS = ∑n(products)S⁰(products) - ∑n(reactants)S⁰(reactants)

     = 1 mole* S°(Br2(g)) - 1 mole*S°(Br2(l))

     =  1 mole *245.5 J/mol-K - 1 mole*152.2 J/mol-K

     = 93.3 J/K

5 0
3 years ago
An unknown amount of helium (He) gas occupies 10.5 L at 1.52 atm pressure and 335 K. What is the mass of helium gas in the conta
Masteriza [31]

Answer:

The lectures in this unit cover gases. This lecture covers the Ideal Gas Law and partial pressures.

Ideal Gas Law

In our previous lecture we discovered a relationship between the pressure, volume, temperature,

and number of moles in gases. After scientists worked out the individual relationships between

pressure, volume, temperature, and the number of moles, it was clear that a single law could

bring all of these individual laws together. This unifying law is called the ideal gas law. An

ideal gas is one which follows the ideal gas law. Not all gases are perfectly ideal in this sense

but most of them are close enough to it that the law applies well.

I. Ideal Gas Law

The Ideal Gas Law unifies all these independent laws as follows:

PV = nRT

Where P = Pressure, V = Volume, T = Temperature, and n = number of moles.

The remaining value, R, is the constant which makes the rest of these factors work together

mathematically. Once the relationship between all individual factors was found it was trivial to

calculate R: it is the value of

PV

nT for any gas since they all act the same way!

There are several numerical values for R depending on which units you are using (atm or torr or

bars, L or mL, Joules (energy) etc). Our class uses this one:

R = .0821

L·atm

mole·K

The ideal gas law helps us calculate variables such as pressure, volume, temperature, or number

of moles without having to make a comparison.

For example, if 3.5 moles O2 has a volume of 27.0 L at a pressure of 1.6 atm, what is the

temperature of the sample?

Here we are given n = 3.5 moles, V = 27.0 L, P = 1.6 atm. We rearrange the ideal gas law to

solve for temperature as follows:

PV = nRT

PV

nR = T

(1.6 atm)(27.0 L)

(3.5 moles)(0.0821 L·atm/mol·K) = 150.3 K

Explanation:

4 0
2 years ago
Read 2 more answers
What causes damage to the ozone layer?
ryzh [129]
<span>Chlorofluorocarbons (CFCs) can damage the ozone layer.</span>
3 0
3 years ago
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Two balloons hold two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can diff
snow_tiger [21]

Answer:

the mass of each gas

Explanation:

Two balloons hold two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can differ between

the two gases?(1 point)

the gas constant of each gas

the molar volume of each gas

the mass of each gas

Two balloons hold two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can differ between the two gases?(1 point) the gas constant of each gas the gas constant of each gas the molar volume of each gas the molar volume of each gas the mass of each gas the mass of each gas the number of moles of each gas

the number of moles of each gas

PV = nRT

The gases have the same P.V, T and n

R is constant AND SO constant for both

the only difference is the molar mass of the gas

for the same number of moles, the  balloons will have different weights depending on the gas  

so the answer is

the mass of each gas

8 0
2 years ago
What is Ka for hno2(aq) = h+(aq) + no2-(aq)?
ikadub [295]
Oxidation number of nitrogen in hno2? ... HNO2, If ON for H: +1. ON for 02: -2 Then (+1) N 2(-2) (+1) N (-4) Therefore Nitrogen's ON is +3.
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