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3 years ago

The maximum number of energy sublevels found in any energy level at ground state is:

Chemistry

2 answers:

algol [13]3 years ago

6 0

Answer:

The maximum number of energy sublevels found in any energy level at ground state is one

Explanation:

The energy state in general can be specified by four quantum numbers:

1) n = principal quantum number = 1,2,3...

2) l = angular momentum where l = 0...n-1

where: l = 0 corresponds the 's' sublevel

l = 1, corresponds to the 'p'

l = 2, corresponds to the 'd' sublevel

3) m = magnetic quantum number which extends from -l....+l

4) s = spin = +1/2 or -1/2

For the ground state n = 1 and l = 0 which corresponds to a single 's' sublevel.

Jlenok [28]3 years ago

4 0

the sublevels of the first four principal energy levels and the maximum number of electrons that the sublevels can contain are summarized in Table 5.1.

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A gas exerts a pressure of 1.8 atm at a temperature of 60 degrees celsius. What is the new temperature when the pressure of the

Kamila [148]

The answer for the following problem is mentioned below.

Therefore the final temperature of the gas is 740 K

Explanation:

Given:

Initial pressure of the gas ( $P_{1}$ ) = 1.8 atm

Final pressure of the gas ( $P_{2}$ ) = 4 atm

Initial temperature of the gas ( $T_{1}$ ) = 60°C = 60 + 273 = 333 K

To solve:

Final temperature of the gas ( $T_{2}$ )

We know;

From the ideal gas equation;

we know;

P × V = n × R × T

So;

we can tell from the above equation;

P ∝ T

(i.e.)

$\frac{P}{T}$ = constant

$\frac{P_{1} }{P_{2} }$ = $\frac{T_{1} }{T_{2} }$

Where;

$P_{1}$ = initial pressure of a gas

$P_{2}$ = final pressure of a gas

$T_{1}$ = initial temperature of a gas

$T_{2}$ = final temperature of a gas

$\frac{1.8}{4}$ = $\frac{333}{T_{2} }$

$T_{2}$ = $\frac{333*4}{1.8}$

$T_{2}$ = 740 K

Therefore the final temperature of the gas is 740 K

8 0

2 years ago

How many moles are in 1.5x1023 molecules of Na2SO4?

german

One mole of Na2SO4 is 6.022 * 10^(23) molecules. We can divide this into the quantity in the question to find a value of 1.5/6.022 = 0.2491 moles. Rounded to two significant figures and put in scientific notation, we can rewrite this quantity as 2.5 * 10^(-1) moles

6 0

1 year ago

The burning of a sample of propane generated 1 04.6 kJ of heat. All of this heat was used to heat 500.0 g of water that had an i

Paul [167]

Answer: 70.0°C

Explanation:

Quantity of heat = Mass * Specific heat * Change in temperature

Quantity of heat = 104.6 KJ

Mass = 500.0 g

Specific heat of water is 4.18 J/g°C

Change in temperature assuming final temperature is x = x - 20

Units should be in grams and joules:

104,600 = 500 * 4.18 * (x - 20)

104,600 = 2,090 * (x - 20)

x - 20 = 104,600/2,090

x = 104,600/2,090 + 20

x = 69.8

= 70.0°C

3 0

3 years ago

The pressure on 30 milliliters of an ideal gas increases from

Nana76 [90]

V1 = 30 mL

P1 = 760 torr

P2 = 1520 torr

V2 = ?

applying Boyle's Law

P1*V1 = P2*V2

760 torr * 30 mL = 1520 torr * V2

V2 = 760 torr * 30 mL / 1520 torr

( C ) is correct

8 0

2 years ago

The carbon dioxide gas that was generated during this reaction was collected at 295K and 125 kPa. If 43.2 L of carbon dioxidegas

Vladimir [108]

Answer:

The balanced equation for this reaction is C2H2 + 502 + 4H2O + 3C02. What volume of carbon dioxide is produced when 2.8 L of oxygen are consumed? 25Explanation:

8 0

2 years ago