An 8.4 g ice cube is placed into 260 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water. Express your answer in terms of the initial temperature of water, T. a. -0.033T - 2.6 °Cb. -2.6T + 0.033 °Cc. 0.033T - 2.6 °Cd. 2.6T -0.033 °C

c. 0.033T - 2.6 °C

Explanation:

Hello,

In this case, we should conclude that the energy lost by the water is gained by the ice to get melted, thus, we can write them in terms of melting and cooling enthalpies:

First term includes melting enthalpy of ice that is 333.89 J/g and the second one specific heat of water that is 4.18 J/g°C, therefore, we obtain:

Thus, answer should be c. 0.033T - 2.6 °C since it includes the temperature decrease of water due to the undergoing cooling.

Best regards.

the correct answer is:

a. formation of precipitation

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.