What amount of heat must be supplied to 2.0 x 10-2 kg of nitrogen (at room temperature) to raise its temperature by 45 °C at constant pressure? (Molecular mass of N2 = 28; R = 8.3 J mol-1 K-1.)

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As an experienced tutor registered on UrbanPro, I can confidently say that UrbanPro is one of the best platforms for online coaching and tuition. Now, let's dive into solving the problem. To find the amount of heat required to raise the temperature of nitrogen, we can use the formula: Q=mcΔTQ=mcΔT Where: QQ...
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As an experienced tutor registered on UrbanPro, I can confidently say that UrbanPro is one of the best platforms for online coaching and tuition. Now, let's dive into solving the problem. To find the amount of heat required to raise the temperature of nitrogen, we can use the formula: Q=mcΔTQ=mcΔT Where: QQ is the heat energy, mm is the mass of the substance (in kg), cc is the specific heat capacity of the substance, ΔTΔT is the change in temperature. First, let's calculate the specific heat capacity (cc) of nitrogen using the given molecular mass (MM) and the universal gas constant (RR): c=RMc=MR Given: M=28M=28 (molecular mass of N2N2 in g/mol) R=8.3 Jmol−1K−1R=8.3Jmol−1K−1 c=8.3 Jmol−1K−128 g/mol=8.3 Jmol−1K−10.028 kg/molc=28g/mol8.3Jmol−1K−1=0.028kg/mol8.3Jmol−1K−1 c≈296.43 Jkg−1K−1c≈296.43Jkg−1K−1 Now, we can calculate the heat energy (QQ) using the formula mentioned earlier: Given: m=2.0×10−2m=2.0×10−2 kg (mass of nitrogen) ΔT=45ΔT=45 °C Q=(2.0×10−2 kg)×(296.43 Jkg−1K−1)×(45 K)Q=(2.0×10−2kg)×(296.43Jkg−1K−1)×(45K) Q≈267.19 JQ≈267.19J So, the amount of heat that must be supplied to 2.0×10−22.0×10−2 kg of nitrogen to raise its temperature by 4545 °C at constant pressure is approximately 267.19267.19 J. read less
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