The amount of heat must be supplied to2.0×10−2kgof nitrogen (at room temperature) to rise its temperature by45∘Cat constant pressure is (Molecular mass ofN2=28;
Question
The amount of heat must be supplied to2.0×10−2kgof nitrogen (at room temperature) to rise its temperature by45∘Cat constant pressure is (Molecular mass ofN2=28;
Solution
To solve this problem, we need to use the formula for heat transfer at constant pressure, which is:
q = m * C_p * ΔT
where:
- q is the heat supplied,
- m is the mass of the substance,
- C_p is the specific heat capacity at constant pressure, and
- ΔT is the change in temperature.
For nitrogen, the specific heat capacity at constant pressure (C_p) is approximately 29.124 J/(mol*K).
First, we need to convert the mass of nitrogen from kg to mol. We know that the molecular mass of N2 is 28 g/mol, so:
2.0 * 10^-2 kg = 2.0 * 10^-2 * 10^3 g = 0.2 g
Therefore, the number of moles (n) is:
n = m/M = 0.2 g / 28 g/mol = 7.14 * 10^-3 mol
Now we can calculate the heat (q):
q = n * C
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