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cupoosta [38]
2 years ago
8

What is the total number of joules released when a 5.00-gram sample of water changes from liquid to solid at 0°C?

Chemistry
1 answer:
Marrrta [24]2 years ago
4 0
Energy released from changing the phase of a substance from the liquid phase to solid phase can be calculated by using the specific latent heat of fusion. The heat of fusion of water at 0 degrees Celsius is 334 J/g. Calculation are as follows:
<span>
Energy = 5 grams x 334 J/g
</span><span>Energy = 1670 J</span>
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A gas effuses 4.0 times faster than oxygen (o2). what is the molecular mass of the gas? 1.0 g/mol 1.0 g/mol 2.0 g/mol 2.0 g/mol
Anastaziya [24]

Answer:

32(molecular mass has no unit )

Explanation:

(16)(o2)

16×2

=32

5 0
2 years ago
An alien civilization has different names and symbols for six elements. Place each element in the correct location in the period
Margarita [4]

Answer:

why whould I know that!!??

Explanation:

3 0
2 years ago
Read 2 more answers
Nitrogen gas reacts with hydrogen gas to produce ammonia. How many liters of hydrogen gas at 95kPa and 15∘C are required to prod
viktelen [127]

Answer:

222.30 L

Explanation:

We'll begin by calculating the number of mole in 100 g of ammonia (NH₃). This can be obtained as follow:

Mass of NH₃ = 100 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3

= 17 g/mol

Mole of NH₃ =?

Mole = mass /molar mass

Mole of NH₃ = 100 / 17

Mole of NH₃ = 5.88 moles

Next, we shall determine the number of mole of Hydrogen needed to produce 5.88 moles of NH₃. This can be obtained as follow:

N₂ + 3H₂ —> 2NH₃

From the balanced equation above,

3 moles of H₂ reacted to produce 2 moles NH₃.

Therefore, Xmol of H₂ is required to p 5.88 moles of NH₃ i.e

Xmol of H₂ = (3 × 5.88)/2

Xmol of H₂ = 8.82 moles

Finally, we shall determine the volume (in litre) of Hydrogen needed to produce 100 g (i.e 5.88 moles) of NH₃. This can be obtained as follow:

Pressure (P) = 95 KPa

Temperature (T) = 15 °C = 15 + 273 = 288 K

Number of mole of H₂ (n) = 8.82 moles

Gas constant (R) = 8.314 KPa.L/Kmol

Volume (V) =?

PV = nRT

95 × V = 8.82 × 8.314 × 288

95 × V = 21118.89024

Divide both side by 95

V = 21118.89024 / 95

V = 222.30 L

Thus the volume of Hydrogen needed for the reaction is 222.30 L

8 0
3 years ago
A sample of methane (CH4) has a volume of 25 mL at a pressure of 0.80 atm. What is the volume of the gas at each of the followin
Xelga [282]

Answer:

a. 50ml b.10ml c. 6.097ml d. 190.1 ml

Explanation:

According to Boyle's law

Volume is inversely proportional to pressure at constant temerature

Mathematically

P1V1=P2V2

P1=Initial pressure=0.8atm

V1=Initial volume=25ml

making V2 the subject

at 0.4atm P2=0.4 atm,

V2=25×0.8/0.4

=50ml

at 2 atm V2=25×0.8/2

=10 ml

1mmHg=0.00131579

2500mmHg=3.28 atm

At 3.28 atm,V2=25×0.8/3.28

=6.097 ml

at 80.0 torr

1 torr=0.00131579

80 torr=0.1052 atm

at 0.1048 atm V2=25×0.8/0.1048

=190.1 ml

4 0
2 years ago
How many grams of CO2 could be formed with 2.09 x 1023 atoms of O?
choli [55]

Answer:

r u in high school this is hard

Explanation:

6 0
3 years ago
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