11/02/17 0 This is a Numeric Entry question /It is worth 1 point/You have unlimi

Question

11/02/17 0 This is a Numeric Entry question /It is worth 1 point/You have unlimited attempts/ o Question (1 point) a See page 236 2nd attempt See Periodic Table See Hint Consider a 55.00 g sample of copper that is cooled from 47.00 to 18.00 ? what is q for this process? The specific heat of solid copper is 0.385 J/gC). Be sure to give your answer the proper sign This amount of heat is used to melt solid ice at O°C. The molar heat of fusion of ice is 6.00 kJ/mol. How many moles of ice are melted? moles 1st attempt 1024 > O OF 24 QUESTIONS COMPLETED arch

Explanation / Answer

cooling is exothermic process. Heat is removed from the substance.

hence Q= heat removed = mass of copper* specific heat* temperature difference = 55*0.385*(47-18)=614 joules

this heat is used to melt ice at 0 deg.c. Heat of fusion of ice= 6KJ/mole= 6*1000j/mole

mole of ice melted= heat removed/ heat of fusion of ice= 614/6000 moles=0.1023 mole

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