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kirill [66]
3 years ago
6

If temperature is kept constant and the volume of a gas is doubled, what will happen to the pressure?

Chemistry
1 answer:
Mrrafil [7]3 years ago
5 0

Answer:

pressure = P1/2

Explanation:

using boyles law

P1V1=P2V2

V2 = 2V1

P1V1=P2 x 2V1

P1 = p2 x 2

P2 = P1/2

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An ionic bond is _?_
lubasha [3.4K]
It would be C, because Ionic bonds have to deal with valence electrons ( the outer shell ones) 
8 0
3 years ago
Which value of x from the set {4, 5, 6, 7), makes this equation true?
irina [24]
C and d is the answer
3 0
3 years ago
Read 2 more answers
How many water molecules does it contain? The density of water is 1.0 g/cm3.
max2010maxim [7]

Complete question is;

A drop of water has a volume of approximately 7 × 10⁻² ml. How many water molecules does it contain? The density of water is 1.0 g/cm³.

This question will require us to first find the number of moles and then use avogadro's number to get the number of water molecules.

<em><u>Number of water molecules = 2.34 × 10²¹ molecules</u></em>

We are given;

Volume of water; V = 7 × 10⁻² ml

Density of water; ρ = 1 g/cm³ = 1 g/ml

Formula for mass is; m = ρV

m = 1 × 7 × 10⁻²

m = 7 × 10⁻² g

from online calculation, molar mass of water = 18.01 g/mol

Number of moles(n) = mass/molar mass

Thus;

n = (7 × 10⁻²)/18.01

n = 3.887 × 10⁻³ mol

from avogadro's number, we know that;

1 mol = 6.022 × 10²³ molecules

Thus,3.887 × 10⁻³ mol will give; 6.022 × 10²³ × 3.887 × 10⁻³ = 2.34 × 10²¹ molecules

Read more at; brainly.in/question/17990661

6 0
3 years ago
Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2
zalisa [80]

Answer:

23.0733 L

Explanation:

The mass of hydrogen peroxide present in 125 g of 50% of hydrogen peroxide solution:

Mass=\frac {50}{100}\times 125\ g

Mass = 62.5 g

Molar mass of H_2O_2 = 34 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus, moles are:

moles= \frac{62.5\ g}{34\ g/mol}

moles= 1.8382\ mol

Consider the given reaction as:

2H_2O_2_{(aq)}\rightarrow2H_2O_{(l)}+O_2_{(g)}

2 moles of hydrogen peroxide decomposes to give 1 mole of oxygen gas.

Also,

1 mole of hydrogen peroxide decomposes to give 1/2 mole of oxygen gas.

So,

1.8382 moles of hydrogen peroxide decomposes to give \frac {1}{2}\times 1.8382 mole of oxygen gas. Moles of oxygen gas produced = 0.9191 molGiven: Pressure = 746 torr&#10;The conversion of P(torr) to P(atm) is shown below:&#10;[tex]P(torr)=\frac {1}{760}\times P(atm)

So,

Pressure = 746 / 760 atm = 0.9816 atm

Temperature = 27 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (27 + 273.15) K = 300.15 K

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.9816 atm × V = 0.9191 mol × 0.0821 L.atm/K.mol × 300.15 K

<u>⇒V = 23.0733 L</u>

8 0
3 years ago
I need Helpppp with my chemistry while we are out of school. I don't have a good teacher and he's not helping since it's his las
9966 [12]

Answer:

im not sure but I hope this helps

Explanation:

I believe the equivalents is just the moles reactant/moles limiting reactant

water has a denisty of 1 g/mL. 1 L is 1000 ml so there are 1000g/L.

the molar mass of water is 18g/mol if you use the Liters in the equation above you can find the number of grams present. divide this number you found by 18 to find the moles.

now take the amount of the other reactant given and divide it by its own molar mass. this will give you the number of moles of that reactant.

divide the moles of water by the moles of the reactant and that is the equivalent.

to find the normality you take this number and divide it by the number of liters.

5 0
3 years ago
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