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vaieri [72.5K]
3 years ago
6

Consider a pot of water at 100 C. If it took 1,048,815 J of energy to vaporize the water and heat it to 135 C, how many grams of

water were in the pot?
Chemistry
1 answer:
jeka57 [31]3 years ago
8 0

Answer:

There was 450.068g of water in the pot.

Explanation:

Latent heat of vaporisation = 2260 kJ/kg = 2260 J/g = L

Specific Heat of Steam = 2.010 kJ/kg C = 2.010 J/g = s

Let m = x g be the weight of water in the pot.

Energy required to vaporise water = mL = 2260x

Energy required to raise the temperature of water from 100 C to 135 C = msΔT = 70.35x

Total energy required = 2260x+x\times2.010\times(135-100)=2260x+70.35x=2330.35x

2330.35x=1048815\\x=450.068g

Hence, there was 450.068g of water in the pot.

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In the given question we need to convert 0.075 meter into centimeter. For this purpose we need to know the relation between meter and centimeter. Then only this problem can be solved and the correct answer reached.
Now we know that
1 meter = 100 centimeter
Then
0.075 meter = [(100/1) * 0.075] centimeter
We know that any number when divided by 1 gives the same number.
So
0.075 meter = (100 * 0.075) centimeter
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How many grams of glucose, C6H12O6, in 2.47 mole?
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First, we need to find the atomic mass of C_{6}H_{12}O_{6}.

According to the periodic table:
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The atomic mass of Oxygen = O = 16

As there are 6 Carbons, 12 Hydrogens and 6 Oxygens, therefore:
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The molar mass of  C_{6}H_{12}O_{6} = 180.156 grams/mole

Now that we have the molar mass of  C_{6}H_{12}O_{6}, we can find the grams of glucose by using:

mass(of glucose in grams) = moles(of glucose given in moles) * molar mass(in grams/mole)

Therefore,
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Ans: Mass of glucose in grams in 2.47 moles = 444.99 grams

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O1Fl2
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