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3 years ago

8

Sue has to find the empirical formula of a compound containing 81.8 grams of carbon and 18.2 grams of hydrogen in 100 grams of c

ompound. What should her first step be?

1 answer:

ArbitrLikvidat [17]3 years ago

6 0

She would divide that mass of each element by it molar mass the answer is C <span />

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The isomerization of cyclopropane to propylene is a first-order process with a half-life of 19 min at 500°c. the time it takes f

amid [387]

<span>As mentioned, the isomerization of cyclopropane to propylene is a first-order process with a half-life of 19 min at 500°c. A first-order reaction kinetic rates means that the rate is constant throughout the reaction.

Thus, the time it takes for the partial pressure of cyclopropane to decrease from 1 atm to 0.125 atm at 500°c is </span><span>57 minutes.</span>

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3 years ago

An object is found to have a mass of 54.3 g. Find the object’s density, if its volume is 47.18 cm3

Schach [20]

Answer:

d≈ 1.15 g/cm^3

Explanation:

The density of an object can be found by dividing the mass over the volume.

d= m/v

The mass of the object is 54.3 grams and the volume is 47.18 cubic centimeters.

m= 54.3 g

v= 47.18 cm^3

Substitute the values into the formula.

d= 54.3 g/ 47.18 cm

Divide.

d= 1.150911403136922 g/cm^3

Let’s round to the nearest hundredth. The 0 in the thousandth place tells us to leave the 5 in the hundredth place.

d ≈ 1.15 g/cm^3

The density is about 1.15 grams per cubic centimeter.

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3 years ago

Calculate the molecular mass of the nonionic solutes.

3241004551 [841]

Answer:

The molecular mass of the nonionic solutes is 124,90 g/m

Explanation:

This is the formula for boiling point elevation.

ΔT = Kb . m

Where ΔT = Tb (solution) - Tb (pure solvent)

Where Kb = the ebullioscopic constant

Where m = molality (moles of solute in 1kg of solvent)

Kb for water is 0,512°C/molal

100,680°C - 100°C = 0,512°C/molal . m

0,680°C = 0,512°C/molal . m

0,680°C /0,512 molal/°C = m

1,32 molality (This are my solute moles in 1kg (1000g) of solvent but I have just 390 g, so let's build the rule of three)

1000 g _____ 1,32 moles

390 g ______ (3,90 g . 1,32 moles) / 1000 g = 0,5148 moles

Molecular mass = g/ mol (mass/moles)

64,3 g /0,5148 moles = 124,90 g/m

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3 years ago

ure to answer all parts. The vapor pressure of ethanol (C2H5OH) at 20°C is 44 mmHg, and the vapor pressure of methanol (CH3OH) a

eimsori [14]

Answer:

$P_{met}=40.98mmHg\\\\P_{et}=24.82mmHg$

Explanation:

Hello

In this case, by considering the Raoult's law we can write:

$P_{met}=x_{met}P_{sat,met}\\\\P_{et}=x_{et}P_{sat,et}$

Whereas the purpose is to compute the pressures of both methanol and ethanol (pressures above the solution), thus, the first step is to compute the molar fractions:

$n_{met}=25.3gCH_3OH*\frac{1molCH_3OH}{32gCH_3OH}=0.791molCH_3OH\\ \\n_{et}=47.1gCH_3CH_2OH*\frac{1molCH_3CH_2OH}{46gCH_3CH_2OH}=1.02molCH_3CH_2OH\\\\x_{met}=\frac{0.791mol}{0.791mol+1.02mol}=0.436\\ \\x_{et}=1-x_{met}=1-0.436=0.564$

Therefore, the pressures turns out:

$P_{met}=0.436*94mmHg=40.98mmHg\\\\P_{et}=0.564*44mmHg=24.82mmHg$

Best regards.

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3 years ago

Which of the following has a dipole moment?

EastWind [94]

Answer:

bb

Explanation:

x yttt fc

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3 years ago