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2 years ago

A gas has a pressure of 500.0 Torr at 35.0 °C. What is the temperature at standard pressure?

Chemistry

1 answer:

Aleks04 [339]2 years ago

5 0

Answer:

466.65 K

Explanation:

Using the formula of Pressure law,

P/T = P'/T'.................... Equation 1

Where P = Intial pressure of gas, T = Initial temperature of gas, P' = Final pressure of gas, T' = Final temperature of gas.

make T' The subeject of equation 1

T' = (P'T)/P................... Equation 2

From the question,

Given: P = 500 Torr = (500×133.322) N/m² = 66661 N/m², T = 35°C = (35+273) = 308 K, P' = 101000 N/m²( Standard pressure)

Substitute these values into equation 2

T' = (101000×308)/66661

T' = 466.65 K

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Calculate the mass of Cr(ClO2)2 that contains 5.57 × 10<br> ^22 chlorine atoms.

Anna007 [38]

Answer:

Explanation:

Your strategy here will be to

use the chemical formula of carbon dioxide to find the number of molecules of

that would contain that many atoms of oxygen

use Avogadro's constant to convert the number of molecules to moles of carbon dioxide

use the molar mass of carbon dioxide to convert the moles to grams

So, you know that one molecule of carbon dioxide contains

one atom of carbon,

two atoms of oxygen,

This means that the given number of atoms of oxygen would correspond to

4.8

⋅

atoms O

⋅

1 molecule CO

atoms O

2.4

⋅

molecules CO

Now, one mole of any molecular substance contains exactly

6.022

⋅

molecules of that substance -- this is known as Avogadro's constant.

In your case, the sample of carbon dioxide molecules contains

2.4

⋅

molecules CO

⋅

1 mole CO

6.022

⋅

molecules CO

0.03985 moles CO

Finally, carbon dioxide has a molar mass of

44.01 g mol

−

, which means that your sample will have a mass of

0.03985

moles CO

⋅

44.01 g

mole CO

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

∣

1.8 g

∣

−−−−−−−−−

The answer is rounded to two sig figs, the number of sig figs you have for the number of atoms of oxygen present in the sample.

3 0

2 years ago

What is the maximum concentration of Ag⁺ that can be added to a 0.00750 M solution of Na₂CO₃ before a precipitate will form? (Ks

Firlakuza [10]

Answer:

$\large \boxed{1.64\times 10^{-5}\text{ mol/L }}$

Explanation:

Ag₂CO₃(s) ⇌2Ag⁺(aq) + CO₃²⁻(aq); Ksp = 8.10 × 10⁻¹²

2x 0.007 50 + x

$K_{sp} =\text{[Ag$^{+}$]$^{2}$[CO$_{3}^{2-}$]} = (2x)^{2}\times 0.00750 = 8.10 \times 10^{-12}\\0.0300x^{2} = 8.10 \times 10^{-12}\\x^{2} = 2.70 \times 10^{-10}\\x = \sqrt{2.70 \times 10^{-10}} = \mathbf{1.64\times 10^{5}} \textbf{ mol/L}\\\text{The maximum concentration of Ag$^{+}$ is $\large \boxed{\mathbf{1.64\times 10^{-5}}\textbf{ mol/L }}$}$

3 0

3 years ago

. What is the mass of 23.56 moles of Glucose<br> ples of Glucose - C6H1206?

GaryK [48]

Answer:

4244.48 g to the nearest hundredth.

Explanation:

The molar mass of Glucose = 6*12.011 + 12*1.008+ 6*15.999

= 180.156.

So 23.56 moles = 180.156 * 23.56 = 4244.48 g

8 0

3 years ago

The height of a wave is called its amplitude. From the noises of the mosquito and the air boat, which aspect of sound is related

TEA [102]

The answer is The loudness of sound is related to its amplitude, this is off edmentum exactly so I advise changing up the wording. You can say something about the pitch or you can word it like, The sound of the wave is related to how loud the sound can be. Hope this helped

3 0

2 years ago

Read 2 more answers

(A tablet containing calcium carbonate and fillers with a mass of 1.631 g was dissolved in HCl. After the fillers were filtered

FrozenT [24]

Answer:

1) 0.825 grams is the mass of pure calcium carbonate product collected at the end of the experiment.

2) The mass % calcium carbonate in the tablet is 50.58%.

3) The mass % of calcium in calcium carbonate is 40.00 %.

4) Mass of calcium in a tablet is 0.33 g.

Explanation:

Mass of tablet = 1.631 g