A 60.0 g sample of chromium at 82.0°C (specific heat for chromium is 0.11 J/g°C) was placed in 80.0 g of water. Assume there is
1 answer:
The temperature of the water and the chromium : 25.122 ° C
<h3>Further explanation </h3>The law of conservation of energy can be applied to heat changes, i.e. the heat received / absorbed is the same as the heat released
Q in(gained) = Q out (lost)
Heat can be calculated using the formula:
Q = mc∆T
Q = heat, J
m = mass, g
c = specific heat, joules / g ° C
∆T = temperature difference, ° C / K
Q Chromium= Q water
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Answer: The mass of the sample will be 1417.7 grams.
Explanation:
We are given:
This means that 1 mole of NaCl has an enthalpy of fusion of 30.2 kJ
1 mole of NaCl has a mass of 58.44 grams.
So, 30.2 kJ of heat is require for a mass 58.44 grams of NaCl
So, 732.6 kJ of heat will be required for = = 1417.65 grams of NaCl.
Hence, the mass of NaCl sample will be 1417.7 grams.
Answer:
2,47 * (molecules)
Explanation:
Avogadro's number is a very important relationship: 1 mole = 6,02 * atoms, molecules, protons, etc.
To convert from moles to molecules, multiply the molar amount by Avogadro's number.
4,1 mol * 6,02 * ≈ 24,7 *
= 2,47 *
(molecules)
Therefore the third answer is correct