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MAVERICK [17]
3 years ago
13

PLS HELPPP

Chemistry
1 answer:
kow [346]3 years ago
4 0
B. 272
I think because it's 3 sig figs 
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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
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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 order to prepare very dilute solutions, a lab technician chooses to perform a series of dilutions instead of measuring a very
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33) How many significant figures does the number 40230 have? *
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Answer:

5

Explanation:

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3 years ago
. Elements are classified as metals, nonmetals, or metalloids according to their
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how much heat is required to raise the temperature of a 5.45-g sample of iron (specific heat = 0.450 j/g°c) from 25.0°c to 79.8°
Mamont248 [21]

Answer:

134.397 Joules

Explanation:

Using the formula:

E = C × m × Δθ (where E is Energy, C is specific heat capacity and Δθ is change in temperature)

So E = 0.45×5.45×(79.8-25)

So E = 134.397 Joules

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2 years ago
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