Calculate the heat required to raise 11b mole of 1-butene at 600°F to 1000°F. Given that Cp=3.909 +62.848x10³ T- 19.617 x 106T² (Cal/gmol°C)

Question 10 please

Use Table B.8 to calculate the energy change, in kJ, as 1 mole of N₂ goes from 800°C to 300°C. The answer must be positive if the substance is heated-up and negative if it is cooled-down.

If a food product is being frozen in a system capable of removing 6200 kJ of thermal energy per product, with the product having a specific heat of 4.1 kJ/kg°C  above the freezing temperature of -1.7°C , a latent heat of fusion of 284 kJ/kg, and the product has a specific heat of 2.2 kJ/kg°C below the freezing temperature. If 10.4 kg of product enters the system at 15°C, and exits it with a temperature of –21 °C, what percentage (to the nearest percent) of the full capability of the freezer has been used?

If 7.08 m3 s-I of air at 322.15 K (50°C) and approximately atmospheric pressure is preheated for a combustion process to 773.15 K (500°C), what rate of heat transfer is required

A food product containing 80% moisture content is being frozen. Estimate the specific heat of the product at -8 ° C when 82% of the water is frozen. The specific heat of the dry product is 2.5 kJ / (kg ° C). it is assumed that the specific heat of water at -10 ° C is the same as the specific heat of water at 0 ° C, and the specific heat of ice follows the function Cp es = 0.0062 Tbeku + 2.0649. Cp frozen product = AnswerkJ / kg ° C.

A food product containing 80% moisture content is being frozen. Estimate the specific heat of the product at -6 ° C when 80% of the water is frozen. The specific heat of the dry product is 2 kJ / (kg ° C). It is assumed that the specific heat of water at -10 ° C is the same as the specific heat of water at 0 ° C, and that the specific heat of ice follows the function Cp es = 0.0062 T frozen + 2.0649. Cp frozen product =    kJ / kg ° C.