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Arisa [49]
3 years ago
8

A balloon occupies a volume of 2.00 l at 40.0oc. how much volume will it occupy at 30.0oc?

Chemistry
1 answer:
hodyreva [135]3 years ago
7 0
<span>Charles' law says "at a constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temperature".

V </span>α T

Where V is the volume and T is the temperature in Kelvin of the gas. We can use this for two situations as,
V₁/T₁ = V₂/T₂

V₁ = 2.00 L
T₁ = 40.0 ⁰C = 313 K
V₂ = ?
T₂ = 30.0 ⁰C = 303 K

By applying the formula,
2.00 L / 313 K = V₂ / 303 K                   
                   V₂ = (2.00 L / 313 K) x 303 K
                   V₂ = 1.94 L

Hence, the volume of the balloon at 30.0 ⁰C  is 1.94 L
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When an electron in an atom spontaneously jumps from a higher energy state to a lower energy state, the atom?
vlabodo [156]
If an atom suffers from a collision, that causes an electron to jump from a lower to higher state, it is called collisional excitation 
6 0
3 years ago
(Thermodynamics)
frutty [35]

Answer:

3853 g

Step-by-step explanation:

M_r: 107.87

         16Ag + S₈ ⟶ 8Ag₂S; ΔH°f =  -31.8 kJ·mol⁻¹

1. Calculate the moles of Ag₂S

Moles of Ag₂S = 567.9 kJ × 1 mol Ag₂S/31.8kJ = 17.858 mol Ag₂S

2. Calculate the moles of Ag

Moles of Ag = 17.86 mol Ag₂S × (16 mol Ag/8 mol Ag₂S) = 35.717 mol Ag

3. Calculate the mass of Ag

Mass of g = 35.717 mol Ag × (107.87 g Ag/1 mol Ag) = 3853 g Ag

You must react 3853 g of Ag to produce 567.9 kJ of heat

3 0
3 years ago
Determine the mole fractions and partial pressures of CO2, CH4, and He in a sample of gas that contains 1.20 moles of CO2, 1.79
BARSIC [14]

Answer :  The mole fraction and partial pressure of CH_4,CO_2 and He gases are, 0.267, 0.179, 0.554 and 1.54, 1.03 and 3.20 atm respectively.

Explanation : Given,

Moles of CH_4 = 1.79 mole

Moles of CO_2 = 1.20 mole

Moles of He = 3.71 mole

Now we have to calculate the mole fraction of CH_4,CO_2 and He gases.

\text{Mole fraction of }CH_4=\frac{\text{Moles of }CH_4}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}

\text{Mole fraction of }CH_4=\frac{1.79}{1.79+1.20+3.71}=0.267

and,

\text{Mole fraction of }CO_2=\frac{\text{Moles of }CO_2}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}

\text{Mole fraction of }CO_2=\frac{1.20}{1.79+1.20+3.71}=0.179

and,

\text{Mole fraction of }He=\frac{\text{Moles of }He}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}

\text{Mole fraction of }He=\frac{3.71}{1.79+1.20+3.71}=0.554

Thus, the mole fraction of CH_4,CO_2 and He gases are, 0.267, 0.179 and 0.554 respectively.

Now we have to calculate the partial pressure of CH_4,CO_2 and He gases.

According to the Raoult's law,

p_i=X_i\times p_T

where,

p_i = partial pressure of gas

p_T = total pressure of gas  = 5.78 atm

X_i = mole fraction of gas

p_{CH_4}=X_{CH_4}\times p_T

p_{CH_4}=0.267\times 5.78atm=1.54atm

and,

p_{CO_2}=X_{CO_2}\times p_T

p_{CO_2}=0.179\times 5.78atm=1.03atm

and,

p_{He}=X_{He}\times p_T

p_{He}=0.554\times 5.78atm=3.20atm

Thus, the partial pressure of CH_4,CO_2 and He gases are, 1.54, 1.03 and 3.20 atm respectively.

4 0
3 years ago
Temperature is a measure of the amount of heat in a substance , true or false
NISA [10]

Answer:

False.

Explanation:

Technically it's false although many people think it is true. The property measured by temperature is Kinetic Energy. Temperature measures how fast particles are moving.

8 0
3 years ago
Read 2 more answers
Place the following transitions of the hydrogen atom in order from longest to shortest wavelength of the photon emitted. Rank fr
gizmo_the_mogwai [7]

Answer:

7 to 4     (higher  \lambda)

5 to 3

3 to 2

4 to 2   (lower  \lambda)

Explanation:

We can use the Rydberg formula which relates the wavelength of the photon emissions to the principle quantum numbers involved in the transition:

\frac{1}{\lambda}=R((\frac{1}{n_1^2})-(\frac{1}{n_2^2}))

with n_1 final n, and n_2 initial n

evaluating for each transition:

7 to 4 \frac{1}{\lambda} = R((\frac{1}{4^2})-(\frac{1}{7^2}))= R(1/16-1/49)=R(0.042)

5 to 3 \frac{1}{\lambda}= R(1/9-1/25)=R(0.071)

4 to 2 \frac{1}{\lambda}= R(1/4-1/16)=R(0.1875)

3 to 2 \frac{1}{\lambda}= R(1/4-1/9)=R(0.139)

Note that the above formula is written for \frac{1}{\lambda}, so lower \frac{1}{\lambda} value obtained involves higher \lambda.

So we should order from lower to higher \frac{1}{\lambda}

7 to 4     (higher  \lambda)

5 to 3

3 to 2

4 to 2   (lower  \lambda)

Note: Take into account that longer wavelength involves lower energy (E=\frac{hc}{\lambda}).

3 0
3 years ago
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