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Pani-rosa [81]
3 years ago
11

How many significant figures are in 5.40

Chemistry
1 answer:
kotykmax [81]3 years ago
4 0
There are 3 significant figures in this value, all values before and after the decimal point are significant. As there is a decimal point, the zeros trailing are also significant.
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0.444 mol C2H5OH= how many molecules
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Explanation:

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Use collision theory to describe the relationship between temperature and volume of a gas.
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3 years ago
A quantity of CO gas occupies a volume of 0.64 L at 0.90 atm and 307 K . The pressure of the gas is lowered and its temperature
levacccp [35]

This is an incomplete question, here is a complete question.

A quantity of CO gas occupies a volume of 0.48 L at 1.6 atm and 282 K. The pressure of the gas is lowered and its temperature is raised until its volume is 2.1 L. Find the density of the CO under the new conditions?

Answer : The density of the CO under the new conditions is, 0.213 g/L

Explanation :

First we have to determine the moles of CO gas by using ideal gas equation.

PV=nRT

where,

P = pressure of gas = 0.90 atm

V = volume of gas = 0.64 L

T = temperature of gas = 3 07 K

R = gas constant = 0.0821 L.atm/mol.K

n = number of moles of gas = ?

Now put all the given values in the above formula, we get:

(0.90atm)\times (0.64L)=n\times (0.0821L.atm/mol.K)\times (307K)

n=0.0228mol

Now we have to calculate the mass of CO gas.

\text{ Mass of }CO=\text{ Moles of }CO\times \text{ Molar mass of }CO

Molar mass of CO = 28g/mole

\text{ Mass of }CO=(0.0228moles)\times (28g/mole)=0.638g

Now we have to calculate the density of CO gas.

\text{Density of CO gas}=\frac{\text{Mass of CO gas}}{\text{Volume of CO gas}}

\text{Density of CO gas}=\frac{0.638g}{3.0L}=0.213g/L

Therefore, the density of the CO under the new conditions is, 0.213 g/L

4 0
3 years ago
Help me I need help with these questions
natali 33 [55]

go to some science website it will help you figure it out if not go to google and look up whatever that is then go to pictures and it will show you.

3 0
3 years ago
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