Answered

A rigid container holds 0.30g of hydrogen gas.
Part A) How much heat is needed to change the temperature of the gas from 50 K to 100 K?
Express your answer to two significant figures and include the appropriate units.
Q= _______
Part B) How much heat is needed to change the temperature of the gas from 250 K to 300 K?
Express your answer to two significant figures and include the appropriate units.
Q=_____
Part C) How much heat is needed to change the temperature of the gas from 2250 K to 2300 K?
Express your answer to two significant figures and include the appropriate units.
Q=_____

Answer :

ajeigbeibraheem

Answer:

Part A:    [tex]\mathbf{Q =94 \ J}[/tex] to two significant figures

Part B:    [tex]\mathbf{Q =160 \ J}[/tex] to two significant figures

Part C:    [tex]\mathbf{Q =220 \ J}[/tex] to two significant figures

Explanation:

Given that :

mass of the hydrogen = 0.30 g

the molar mass of hydrogen gas molecule = 2 g/mol

we all know that:

number of moles = mass/molar mass

number of moles = 0.30 g /2 g/mol

number of moles = 0.15 mol

For low temperature between the range of 50 K to 100 K, the specific heat at constant volume for a diatomic gas molecule = [tex]C_v=\dfrac{3}{2}R[/tex]

For Part A:

[tex]Q = mC_v\Delta T[/tex]

[tex]Q= 0.15 \ mol (\dfrac{3}{2})(8.314 \ J/mole.K )(100-50)K[/tex]

[tex]Q= 0.15 \times (\dfrac{3}{2}) \times (8.314 \ J )\times (50)[/tex]

[tex]Q=93.5325 \ J[/tex]

[tex]\mathbf{Q =94 \ J}[/tex] to two significant figures

Part B. For hot temperature, [tex]C_v=\dfrac{5}{2}R[/tex]

[tex]Q = mC_v\Delta T[/tex]

[tex]Q= 0.15 \ mol (\dfrac{5}{2})(8.314 \ J/mole.K )(300-250)K[/tex]

[tex]Q= 0.15 \times (\dfrac{5}{2}) \times (8.314 \ J )\times (50)[/tex]

[tex]Q=155.8875 \ J[/tex]

[tex]\mathbf{Q =160 \ J}[/tex] to two significant figures

Part C. For an extremely hot temperature, [tex]C_v=\dfrac{7}{2}R[/tex]

[tex]Q = mC_v\Delta T[/tex]

[tex]Q= 0.15 \ mol (\dfrac{7}{2})(8.314 \ J/mole.K )(2300-2250)K[/tex]

[tex]Q= 0.15 \times (\dfrac{7}{2}) \times (8.314 \ J )\times (50)[/tex]

[tex]Q=218.2425 \ J[/tex]

[tex]\mathbf{Q =220 \ J}[/tex] to two significant figures

Part A)  Heat needed to change the temperature of the gas from 50 K to 100 K is 94J.

Part B) Heat needed to change the temperature of the gas from 250 K to 300 K is 160J.

Part C) Heat needed to change the temperature of the gas from 2250 K to 2300 K is 220J.

What is heat?

The increment in temperature adds up the thermal energy into the object. This energy is Heat energy.

Given is the mass of the hydrogen = 0.30 g and the molar mass of hydrogen gas molecule = 2 g/mol

Then, number of moles = mass/molar mass

number of moles = 0.30 g /2 g/mol = 0.15 mol

Part A) For low temperature between the range of 50 K to 100 K, the specific heat at constant volume for a diatomic gas molecule Cv =3/2R

Q =m Cv ΔT

Q = 0.15 mol x 3/2 x 8.314 x (100 - 50)

Q = 93.5325 Joules.

Q = 94 J to two significant figures.

Part B) For hot temperature, Cv = 5/2 R

Heat needed, Q =m Cv ΔT

Q = 0.15 mol x 5/2 x 8.314 x (300 - 250)

Q = 155.8875Joules.

Q = 160 J to two significant figures.

Part C) In case of extremely hot temperature, Cv =7/2R

Heat needed to change the temperature from 2250 K to 2300 K

Q = 0.15 mol x 7/2 x 8.314 x (2300 - 2250)

Q = 218.2425 J

Q = 220J

Learn more about heat.

https://brainly.com/question/13860901

#SPJ5

Other Questions