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Harlamova29_29 [7]
2 years ago
15

DOES ANYONE KNOW THE ANSWER?

Chemistry
1 answer:
Yanka [14]2 years ago
3 0

Answer:

You can only be able to solve two variables, k and x based on what you input as your question

k= -2x+3

x= (3-k)/2

Explanation:

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d

Explanation:

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Why is snow a better insulator than ice?
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Snow is a better insulator than ice because snow contains air packets inside it and air is a good insulator of heat. Due to this, snow takes longer time to melt than the ice of the same mass.

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7 0
3 years ago
A gas has a volume of 5.0 L at a pressure of 50 KPa. What happens to the volume when the pressure is increased to 125?
Alexeev081 [22]
The volume becomes two. You have to use the equation P1 x V1 = P2 x V2 
P is pressure and V is volume.
P1 = 50     P2 = 125
V1 = 5       V2 = v (we don't know what it is)
Then set up the equation:
50 times 5 = 125 times v
250 = 125v
the divide both sides by 125 and isolate v
2 = v
Therefore the volume is decreased to 2.
Also, Boyle's Law explains this too: Volume and pressure are inversely related, This means that when one goes up the other goes down (ie when pressure increases volume decreases and vice versa). Becuase the pressure went up from 50 KPa tp 125 KPa the volume had to decrease.

7 0
3 years ago
The heat of combustion of ethane is -337.0kcal at 25 degrees celsius. what is the heat of the reaction when 3g of ethane is burn
Ghella [55]

Answer:

Q = -33.6kcal .

Explanation:

Hello there!

In this case, according to the equation for the calculation of the total heat of reaction when a fixed mass of a fuel like ethane is burnt, we can write:

Q=n*\Delta _cH

Whereas n stands for the moles and the other term for the enthalpy of combustion. Thus, for the required total heat of reaction, we first compute the moles of ethane in 3 g as shown below:

n=3g*\frac{1mol}{30.08g}=0.1mol

Next, we understand that -337.0kcal is the heat released by the combustion of 1 mole of ethane, therefore, to compute Q, we proceed as follows:

Q=0.1mol*-337.0\frac{kcal}{mol}\\\\Q=-33.6kcal

Best regards!

8 0
3 years ago
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