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3 years ago

What volume (in L) of ethane (C2H6) will be required to produce 42.5 L of carbon dioxide in the reaction below?

Chemistry

2 answers:

Luda [366]3 years ago

4 0

Answer:

21.25

Explanation:

Nana76 [90]3 years ago

3 0

Answer:

23.4

Explanation:

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The flow of energy in an ecosystem starts with

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From the sun, through the photosynthetic organisms which includes; green plants and algae, then to herbivores to carnivores and decomposers.

I hope this helps answer your question. <3

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3 years ago

All of the covalent carbon-carbon bonds in unsaturated hydrocarbons share 2 pairs of electrons.

Evgen [1.6K]

False. carbon-carbon bonds that share 2 pairs of electrons are double bonds. An unsaturated hydrocarbon isnt necessary to only have double bonds. they can also have single bonds or triple bonds.

5 0

3 years ago

Read 2 more answers

Phenolphthalein is an indicator that turns from colorless (acidic form) to magenta (basic form) and has a pKa of 9.40. What is t

frosja888 [35]

Answer:

40:1 is the ratio of the magenta phenolphthalein concentration to the colorless phenolphthalein concentration.

Explanation:

To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

$pH=pK_a+\log(\frac{[salt]}{[acid]})$

$pH=pK_a+\log(\frac{[magenta(Php)]}{[Php]})$

We are given:

$pK_a$ = negative logarithm of acid dissociation constant of phenolphthalein = 9.40

$[magenta(Php)]$ = concentration of magenta phenolphthalein

$[Php]$ = concentration of colorless phenolphthalein

pH = 11

Putting values in above equation, we get:

$11=9.40+\log(\frac{[magenta(Php)]}{[Php]})$

$\log(\frac{[magenta(Php)]}{[Php]})=11-9.40=1.6$

$\frac{[magenta(Php)]}{[Php]}=10^{1.6}=39.81 :1 \approx 40:1$

40:1 is the ratio of the magenta phenolphthalein concentration to the colorless phenolphthalein concentration.

7 0

3 years ago

How many grams of methane should be burned in an excess of oxygen at STP to obtain 5.6 L of carbon dioxide?

Mars2501 [29]

The balanced chemical reaction would be as follows:

CH4 + O2 = CO2 + 2H2O

We are given the amount of CO2 product in the reaction. This will be the starting point for the calculations. We do as follows:

5.6 L CO2 ( 1 mol / 22.4L ) ( 1 mol CH4 / 1 mol CO2 ) ( 16.05 g / 1 mol ) = 4.01 g CH4 needed

6 0

3 years ago

Read 2 more answers

A chemist conducts an experiment in which 2.0 L of hydrogen gas is collected over water at 1 atm and 298 K. Remember the pressur

Studentka2010 [4]

Answer:

$V_2=1.80L$

Explanation:

Hello!

In this case, since in this problem we can see that the volume, pressure and temperature are changing, considering that the vapor pressure of water at 0 °C or also 273 K is 0.006 atm, the pressure of dry hydrogen would be 0.99 atm, thus, we can write:

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

Now, as we need the final volume V2, by solving for it, we write:

$V_2=\frac{P_1V_1T_2}{T_1P_2}$

In such a way, we plug in the given data to obtain:

$V_2=\frac{0.97atm*2.0L*273K}{298K*0.99atm}\\\\V_2=1.80L$

Which means that the underwent a compression.

Best regards!

4 0

3 years ago