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3 years ago

When using 100ml or 50ml graduated cylinder to what decimal place can your volume be estimated?

Chemistry

1 answer:

Olegator [25]3 years ago

3 0

Answer:

I know that the 100-mL graduated cylinders are always read to 1 decimal place.

I think for 50 mL graduated cylinders, it lets you measure volumes up to 50.0 mL to the nearest 0.1 or 0.2 mL, depending on your exact cylinder.

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3 years ago

Suppose that the volume of a particular sample of Cl2 is 718 mL at 675 mmHg and 48C at what temperature in C will the volume be

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Answer:

1900 °C

Step-by-step explanation:

This looks like a case where we can use the Combined Gas Law to calculate the temperature.

p₁V₁/T₁ = p₂V₂/T₂ Multiply both sides by T₂

p₁V₁T₂/T₁ = p₂V₂ Multiply each side by T₁

p₁V₁T₂ = p₂V₂T₁ Divide each side by p₁V₁

T₂ = T₁ × p₂/p₁ × V₂/V₁

=====

Data:

We must convert the pressures to a common unit. I have chosen atmospheres.

p₁ = 675 mmHg × 1atm/760 mmHg = 0.8882 atm

V₁ = 718 mL = 0.718 L

T₁ = 48 °C = 321.15 K

p₂ = 159 kPa × 1 atm/101.325 kPa = 1.569 atm

V₂ = 2.0 L

T₂ = ?

=====

Calculation:

T₂ = 321.15 × 1.569/0.8882 × 2.0/0.718

T₂ = 321.15 × 1.766 × 2.786

T₂ = 321.15 × 1.569/0.8882 × 7.786

T₂ = 1580K

T₂ = 1580 + 273.15

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Note: The answer can have only two significant figures because that is all you gave for the second volume of the gas.

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3 years ago

Calculate the following quantity: volume of 1.403 M copper(II) nitrate that must be diluted with water to prepare 575.2 mL of a

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Answer:

328 ml

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We have given final volume =575.2 ml=0.575 L

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We know that moles of copper(II) nitrate = final volume ×final concentration =0.8012×.0575=0.4606 moles

We have to find initial volume

So initial volume $=\frac{moles\ of \ copper(II)\ nitrate}{initial\ concentration}=\frac{0.4606}{1.403}=0.328L=328ml$

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When using 100ml or 50ml graduated cylinder to what decimal place can your volume be estimated?​

When using 100ml or 50ml graduated cylinder to what decimal place can your volume be estimated?