Calculate the energy needed to raise the temperature of 18.0g of water from 10.0C to 40.0C. The specific heat of water is 4.18 J
1 answer:
Answer:
The energy needed to raise the temperature 18.0 grams of water is from 10.0°C to 40.0°C is 2,257.2 Joules.
Explanation:
Where:
Q = heat absorbed or heat lost
c = specific heat of substance
m = Mass of the substance
ΔT = change in temperature of the substance
: Initial and final temperature of the substance
We have mass of water = m = 18.0 g
Specific heat of water= c = 4.18 J/g°C
Initial and final temperature of the water=
Final temperature of the water=
Heat absorbed by the water:
The energy needed to raise the temperature 18.0 grams of water is from 10.0°C to 40.0°C is 2,257.2 Joules.
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Answer: 0.20 M
Explanation:
According to the dilution law,
where,
= molarity of stock solution = 1.40 M
= volume of stock solution = 72.0 ml
= molarity of diluted solution = m
= volume of diluted solution = 248 ml
Now 124 mL portion of this prepared solution is diluted by adding 133 mL of water.
According to the dilution law,
where,
= molarity of stock solution = 0.41 M
= volume of stock solution = 124 ml
= molarity of diluted solution = m
= volume of diluted solution = (124 +133) ml = 257 ml
Thus the final concentration of the solution is 0.20 M.