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3 years ago

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What colour is the flame

1 answer:

maks197457 [2]3 years ago

8 0

I can't see an image but I'm guessing red, yellow, or orange.

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10 pointsss Where are tsunamis likely to originate?

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Tsunamis are likely to originate in the pacific ocean

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3 years ago

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Please help me i will give brain list tap the question

mr_godi [17]

Answer:

molecular formulas of the hydrocarbons

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3 years ago

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1- A sample of gas is in a 3.00 L contain at a pressure of 740.0 mmHg. What is the new pressure of the sample if the container's

inna [77]

Considering the Boyle's law, the new pressure of the sample is 1,776 mmHg.

<h3>What is Boyle's law</h3>

Boyle's law establishes the relationship between the pressure and the volume of a gas when the temperature is constant.

Boyle's law states that the volume occupied by a given mass of gas at constant temperature is inversely proportional to the pressure. This means that if the pressure increases, the volume decreases, while if the pressure decreases, the volume increases.

Boyle's law is expressed mathematically as:

P×V=k

Now it is possible to assume that you have a certain volume of gas V1 which is at a pressure P1 at the beginning of the experiment. If you vary the volume of gas to a new value V2, then the pressure will change to P2, and the following will be true:

P1×V1=P2×V2

<h3>New pressure</h3>

In this case, you know:

P1= 740 mmHg
V1= 3 L
P2= ?
V2= 1.25 L

Replacing in Boyle's law:

740 mmHg× 3 L=P2× 1.25 L

Solving:

P2= (740 mmHg× 3 L) ÷ 1.25 L

P2= 1,776 mmHg

Finally, the new pressure of the sample is 1,776 mmHg.

Learn more about Boyle's law:

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2 years ago

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What state is lake erie

svetoff [14.1K]

Lake Erie is bordered by four states: New York, Ohio, Pennsylvania and Michigan.

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3 years ago

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The combustion of how many moles of ethane (C2H6) would be required to heat 851 g of water from 25.0°C to 98.0°C? (Assume liquid

Debora [2.8K]

Answer : The number of moles of ethane required will be 0.166 mole.

Explanation :

First we have to calculate the heat absorbed by water.

$q=m\times c\times (T_{final}-T_{initial})$

where,

q = heat absorbed = ?

m = mass of water = 851 g

c = specific heat of water = $4.18J/g^oC$

$T_{final}$ = final temperature = $98.0^oC$

$T_{initial}$ = initial temperature = $25.0^oC$

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

$q=851g\times 4.18J/g^oC\times (98.0-25.0)^oC$

$q=259674.14J=259.67kJ$ (1 kJ = 1000 J)

Now we have to calculate the moles of ethane required.

$\Delta H=\frac{q}{n}$

where,

$\Delta H$ = enthalpy of combustion of ethane = 1560.7 kJ/mol (standard value)

q = heat absorbed = 259.67 kJ

n = number of moles of ethane = ?

$1560.7kJ/mol=\frac{259.67kJ}{n}$

$n=\frac{259.67kJ}{1560.7kJ/mol}$

$n=0.166mole$

Therefore, the number of moles of ethane required will be 0.166 mole.

8 0

3 years ago