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maw [93]
2 years ago
14

Calculate the density of a material that has mass of 52.457g and a volume of 13.5 cm3

Chemistry
1 answer:
Nesterboy [21]2 years ago
5 0
1 cm3 = 1 ml
Density is g/ml

So this is 52.457g / 13.5ml = 3.89 g/ml
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Base

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What is the absorbance of the permanganate in the diluted waste solution?
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Now, examine the structures of benzhydrol and fluorene. Both compounds contain the same number of carbons but have very differen
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The OH group

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How many grams of KCl 03 are needed to produce 6.75 Liters of O2 gas measured at 1.3 atm pressure and 298 K?
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11.48-gram of KCl0_3 are needed to produce 6.75 Liters of O_2  gas measured at 1.3 atm pressure and 298 K

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

First, calculate the moles of the gas using the gas law,

PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= 1.3 atm

V= 6.75 Liters

n=?

R= 0.082057338 \;L \;atm \;K^{-1}mol^{-1}

T=298 K

Putting value in the given equation:

\frac{PV}{RT}=n

n= \frac{1.3 \;atm\; X \;6.75 \;L}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 298}

Moles = 0.3588 moles

Now,

Moles = \frac{mass}{molar \;mass}

0.3588 moles = \frac{mass}{32}

Mass= 11.48 gram

Hence, 11.48-gram of KCl0_3 are needed to produce 6.75 Liters of O_2 gas measured at 1.3 atm pressure and 298 K

Learn more about the ideal gas here:

brainly.com/question/27691721

#SPJ1

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