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Nezavi [6.7K]
3 years ago
9

I bet half these people are kids from lhs rite now lol

Chemistry
2 answers:
Nana76 [90]3 years ago
7 0
I bet that half of them can type or write better than you can.
Sunny_sXe [5.5K]3 years ago
3 0
No not really this is a global thing millions use this
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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?
Nina [5.8K]

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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How many atoms of Lead are in a 62.7 g sample of Lead(II) permanganate?
Alexandra [31]

Answer:

\large \boxed {8.48 \times 10^{22}\text{ atoms}}

Explanation:

1 mol of Pb(MnO₄)₂contains 1 mol of Pb atoms.

1. Moles of Pb

\text{Moles of Pb} = \text{62.7 g Pb(MnO$_{4}$)}_{2} \times \dfrac{\text{1 mol Pb(MnO$_{4}$)}_{2}}{\text{445.07 g Pb(MnO$_{4}$)}_{2}}\\\\\times \dfrac{\text{1 mol Pb}}{\text{1 mol  Pb(MnO$_{4}$)}_{2}} = \text{0.1409 mol Pb}

2. Atoms of Pb

\text{Atoms of Pb} = \text{0.1409 mol Pb } \times \dfrac{ 6.022  \times 10^{23}\text{ atoms Pb }}{\text{1 mol Pb }}\\\\= \large \boxed {\mathbf{8.48 \times 10^{22}}\textbf{ atoms Pb }}

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