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Setler [38]
3 years ago
14

Determine the heat energy needed to raise the temperature of 120 grams of ice at -5 to steam at 115°

Chemistry
1 answer:
CaHeK987 [17]3 years ago
5 0

Answer:

Q = 30355.2 J

Explanation:

Given data:

Mass of ice = 120 g

Initial temperature = -5°C

Final temperature = 115°C

Energy required = ?

Solution:

Specific heat capacity of ice is = 2.108 j/g.°C

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

Q = m.c. ΔT

ΔT = T2 -T1

ΔT = 115 - (-5°C)

ΔT = 120 °C

Q = 120 g × 2.108 j/g.°C × 120 °C

Q = 30355.2 J

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Transport of aspirin is expected to be faster in the ____. The speed of nonmediated absorption depends strongly on the polarity
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Answer:

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Explanation:

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7 0
3 years ago
0.055 grams of PbSO4 is dissolved in 200.00 grams of H2O.
Greeley [361]

Answer:

Solution's mass = 200.055 g

[PbSO₄] = 275 ppm

Explanation:

Solute mass = 0.055 g of lead(II) sulfate

Solvent mass = 200 g of water

Solution mass = Solvent mass + Solution mass

0.055 g + 200 g = 200.055 g

ppm = μg of solute / g of solution

We convert the mass of solute from g to μg

0.055 g . 1×10⁶ μg/ 1g = 5.5×10⁴μg

5.5×10⁴μg / 200.055 g = 275 ppm

ppm can also be determined as mg of solute / kg of solution

It is important that the relation is 1×10⁻⁶

Let's verify: 0.055 g = 55 mg

200.055 g = 0.200055 kg

55 mg / 0.200055 kg = 275 ppm

6 0
3 years ago
Convert 3.01 x 10^24 molecules of ammonium sulfate to mass
Dmitry [639]

Mass  of ammonium sulfate = 660.7 g

<h3>Further explanation</h3>

Given

3.01 x 10²⁴ molecules of ammonium sulfate

Required

mass

Solution

The mole is the number of particles(molecules, atoms, ions) contained in a substance  

1 mol = 6.02.10²³ particles

Can be formulated

N=n x No

N = number of particles

n = mol

No = Avogadro's = 6.02.10²³

mol ammonium sulfate (NH₄)₂SO₄ :

n = N : No

n = 3.01 x 10²⁴ : 6.02 x 10²³

n = 5

mass ammonium sulfate :

= mol x MW

= 5 x 132,14 g/mol

= 660.7 g

5 0
3 years ago
The picture has my question
aleksandr82 [10.1K]

Answer:

b or c

Explanation:

5 0
2 years ago
Read 2 more answers
What mass of H₂O is formed when excess H₂ reacts with 64 g of O₂
taurus [48]

Answer: 72 g of H_2O is formed.

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} O_2=\frac{64}{32}=2moles

2H_2+O_2(g)\rightarrow 2H_2O

As  H_2 is the excess reagent, O_2 is the limiting reagent as it limits the formation of product.

According to stoichiometry :

1 mole of O_2 produce=  2 moles of H_2O

Thus 2 moles of O_2 will require=\frac{2}{1}\times 2=4moles  of H_2O

Mass of H_2O=moles\times {\text {Molar mass}}=4moles\times 18g/mol=72g

Thus 72 g of H_2O is formed.

4 0
2 years ago
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