What amount of heat is needed to raise the temperature of $$2$$×$$10-2$$ kg of nitrogen at room temperature to raise it’s temperature by $$45$$° C at constant pressure?(given$$ molecular $$mass=28$$ and $$R=8.3$$ J $$mol-1$$ $$K-1$$; $$Cp=7R/2)

Question

What amount of heat is needed to raise the temperature of $$2$$×$$10-2$$ kg of nitrogen at room temperature to raise it’s temperature by $$45$$° C at constant pressure?(given$$ molecular $$mass=28$$ and  $$R=8.3$$ J $$mol-1$$ $$K-1$$;  $$Cp=7R/2)

Infinity Learn · Accepted Answer

number of $$molesn=mM=2028=0.174where$$ m is mass of gas in $$gram=0.02kg=0.02x1000g=20gM$$ is molecular weight of gas  molar specific heat of gas at constant pressure is Cp  $$Cp=7R/2=72$$×$$8.3$$ J $$mole-1$$ K−$$1$$  amount of heat required to raise temperature of gas at constant pressure is Q  $$Q=nCp$$×ΔT  here ΔT is raise in temperature  substitute the values of n,Cp,ΔT  $$Q=0.714$$×$$72$$×$$8.3$$ ×$$45$$ J ⇒$$Q=933.75J$$

What amount of heat is needed to raise the temperature of $2 \times 10^{- 2} k g$ of nitrogen at room temperature to raise it’s temperature by 45° C at constant pressure?(given molecular mass=28 and R=8.3 J $m o l^{- 1} K^{- 1}$ ; $C_{p} =7R/2$ )

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What amount of heat is needed to raise the temperature of 2×10-2 kg of nitrogen at room temperature to raise it’s temperature by 45° C at constant pressure?(given molecular mass=28 and R=8.3 J mol-1 K-1; Cp=7R/2)

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What amount of heat is needed to raise the temperature of $2 \times 10^{- 2} k g$ of nitrogen at room temperature to raise it’s temperature by 45° C at constant pressure?(given molecular mass=28 and R=8.3 J $m o l^{- 1} K^{- 1}$ ; $C_{p} =7R/2$ )