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3 years ago

I need help ASAP!!!!! What happens to water when it changes to ice?

Chemistry

2 answers:

Gre4nikov [31]3 years ago

6 0

- It's density increases

- mass increases

- volume increases

Hope this helps!

xenn [34]3 years ago

6 0

Answer:

first one

Explanation:

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The movement of atoms molecules waves and electrons is

nikdorinn [45]

Energy, I think, haven't done that since 8th grade

4 0

3 years ago

A 1. 00 ml sample of an unknown gas effuses in 11. 1 min. an equal volume of h2 in the same apparatus under the same conditions

Damm [24]

A 1. 00 ml sample of an unknown gas effuses in 11. 1 min. an equal volume of h2 in the same apparatus under the same conditions effuses in 2. 42 minutes then the molar mass of the unknown gas is 41.9.

Molar mass of H2 = 2

Molar mass of unknown gas = ?

rate 1 = 11.1

rate 2 = 2.42

<h3>What is graham law? </h3>

Graham's law states that the rate of diffusion or effusion of a given gas is inversely proportional to the square root of its molar mass.

By apply graham law

Rate1/rate2 = sqrt(MW2/MW1)

$[\frac{rate1}{rate2} ]^{2} = \frac{MW2}{2} \\\\\\mw= 2[\frac{11.1}{2.42} ]^{2} \\\\= 20.97 X 2 \\\\= 41.9$

Thus, we found that the molar mass of the unknown gas is 41.9.

Learn more about graham's law: brainly.com/question/12415336

#SPJ4

4 0

2 years ago

Butane, ch3-ch2-ch2-ch3, is a hydrocarbon fuel used in lighters. how many moles of molecules are there in a 350. gram sample of

Galina-37 [17]

<span>6.03 moles.

1 molecule of butane contains 4 carbon atoms and ten hydrogen atoms.

The molar mass is 4 times the atomic mass of carbon, 12 g/mol, plus 10 times the atomic weight of hydrogen, 1 g/mol.

Molar mass = 4 * 12 g/mol + 10 * 1 g/mol = 58 g/mol.

This means that 1 mole of butane has a mass of 58 g.

To figure out how many moles are in a sample of butane, divide the mass of sample in grams by 58 grams

Number of moles in sample = 350 g / 58 g/mol = 6.03 moles.</span>

3 0

3 years ago

Which of earth's spheres is most affected by weathering and erosion

Natali [406]

Answer: the hydrosphere

Explanation:

3 0

3 years ago

Determine the mass of CaCO3 required to produce 40.0 mL CO2 at STP. Hint use molar volume of an ideal gas (22.4 L)

cupoosta [38]

Answer:

$m_{CaCO_3}=0.179gCaCO_3$

Explanation:

Hello,

In this case, since the undergoing chemical reaction is:

$CaCO_3(s)\rightarrow CaO(s)+CO_2(g)$

The corresponding moles of carbon dioxide occupying 40.0 mL (0.0400 L) are computed by using the ideal gas equation at 273.15 K and 1.00 atm (STP) as follows:

$PV=nRT\\\\n=\frac{PV}{RT}=\frac{1.00 atm*0.0400L}{0.082\frac{atm*L}{mol*K}*273.15 K})=1.79x10^{-3} mol CO_2$

Then, since the mole ratio between carbon dioxide and calcium carbonate is 1:1 and the molar mass of the reactant is 100 g/mol, the mass that yields such volume turns out:

$m_{CaCO_3}=1.79x10^{-3}molCO_2*\frac{1molCaCO_3}{1molCO_2} *\frac{100g CaCO_3}{1molCaCO_3}\\ \\m_{CaCO_3}=0.179gCaCO_3$

Regards.

3 0

3 years ago