1 g of water at 100° C is completely converted into steam at 100° C. 1 g of steam occupies a volume of 1650 cc. (Neglect the volume of 1 g of water at 100° C ). At the pressure of 105 N / m 2, latent heat of steam is 540 cals / g (1 calorie =4.2 joule). The increase in the internal energy (in joule) is

Question

1 g of water at 100° C is completely converted into steam at 100° C. 1 g of steam occupies a volume of 1650 cc. (Neglect the volume of 1 g of water at 100° C ). At the pressure of 105 N / m 2, latent heat of steam is 540 cals / g (1 calorie =4.2 joule). The increase in the internal energy (in joule) is (A) 2310 (B) 2203 (C) 1650 (D) 2150

Tardigrade Admin · Accepted Answer

Heat required to convert 1 g of water at 100° C completely into steam at 100° C d Q=m L =1 × 540 calorie =540 × 4.2=2268 J Work done in expanding volume d W =p d V=105(V2-V1) =105(1650-1000) × 106 =650 × 10-1=65 Increase in internal energy d U=d Q-d W=2268-65=2203 J

Q. 1g of water at 100∘C is completely converted into steam at 100∘C. 1g of steam occupies a volume of 1650cc. (Neglect the volume of 1g of water at 100∘C ). At the pressure of 105N/m2, latent heat of steam is 540cals/g (1 calorie =4.2 joule). The increase in the internal energy (in joule) is

2310

2203

1650

2150

Heat required to convert 1g of water at 100∘C completely into steam at 100∘C dQ=mL =1×540 calorie =540×4.2=2268J Work done in expanding volume dW=pdV=105(V2​−V1​) =105(1650−1000)×106 =650×10−1=65 Increase in internal energy dU=dQ−dW=2268−65=2203J