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Charra [1.4K]
3 years ago
6

During one researcher's experiment, the total mass of the gas-generating solid and entire assembly was 52.1487g before the react

ion and 52.1098g after the reaction. If the number of moles of gas generated was calculated to be 8.854 x 10-4 mol, what is the molar mass of the gas?
Chemistry
1 answer:
irinina [24]3 years ago
7 0

Answer:

43.93 g/mol

Explanation:

The mass of the gas before reaction = 52.1487 g

The mass of the gas after reaction = 52.1098 g

Mass of gas generated = 0.0389 g

Moles of the gas = 8.854\times 10^{-4}\ moles

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Molar\ mass = \frac{Mass\ taken}{Moles}

Molar\ mass= \frac{0.0389\ g}{8.854\times 10^{-4}\ moles}

Molar mass of the gas = 43.93 g/mol

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Q = 114349.5 J

Explanation:

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In this case, since this a problem in which we need to calculate the total heat of the described process, it turns out convenient to calculate it in three steps; the first one, associated to the heating of the liquid water from 40 °C to 100 °C, next the vaporization of liquid water to steam at constant 100 °C and finally the heating of steam from 100 °C to 115 °C. In such a way, we calculate each heat as shown below:

Q_1=45g*4.18\frac{J}{g\°C}*(100\°C-40\°C)=11286J\\\\Q_2=45g* 2260 \frac{J}{g} =101700J\\\\Q_3=45*2.02\frac{J}{g\°C}*(115\°C-100\°C)=1363.5J

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3 years ago
If 60. liters of hydrogen gas at 546 K is cooled to 273 K at constant pressure, the new volume of the gas would be
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Explanation:

Initial Volume

=

V

1

=

60

l

i

t

e

r

Initial Temperature

=

T

1

=

546

K

Final Temperature

=

T

2

=

273

K

Final Vloume

=

V

2

=

?

?

Sol:-

Since the pressure is constant and the question is asking about temperature and volume, i.e,

V

1

T

1

=

V

2

T

2

⇒

V

2

=

V

1

⋅

T

2

T

1

=

60

⋅

273

546

=

60

2

=

30

l

i

t

e

r

⇒

V

2

=

30

l

i

t

e

r

Hence the new volume of the gas is

30

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i

t

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r

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