The enthalpy change upon dissolving 80 grams of ammonium nitrate in water is +25.7 kJ. Will the solution feel cold or warm to touch? Group of answer choiceswarmcold

The enthalpy change upon dissolving 80 grams of ammonium nitrate in water is +25.7 kJ. If 160 grams are dissolved, what will be the change in enthalpy? Group of answer choicesNot enough information to tellIt will be halvedIt will be doubled

A student dissolves 14.5 g of ammonium nitrate NH4NO3 in 250. g of water in a well-insulated open cup. She then observes the temperature of the water fall from 20.0 °C to 16.5 °C over the course of 8.1 minutes.Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction:→NH4NO3s + NH+4aq  NO−3aqYou can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits.Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction.Is this reaction exothermic, endothermic, or neither? exothermicendothermicneitherIf you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJCalculate the reaction enthalpy ΔHrxn per mole of NH4NO3. kJmol

When ammonium nitrate, NH4NO3(s) is added to water at 25 °C, it dissolves spontaneously and the temperature of the solution decreases. This indicates that the factor causing the substance to dissolve is a change in ________.Group of answer choicestemperatureenergyenthalpyentropy

If 0.241mol of ammonium chloride NH4Cl is dissolved in a liquid producing ×−2.43102cal of heat, calculate the temperature change of ×6.51102g of the resulting solution if the specific heat capacity of the solution is 0.800cal·g°C. Round your answer to 3 significant figures.

Liam investigates the energy released when ammonium nitrate is dissolved in water.His method is as follows:Liam’s results were:Initial temperature = 20 ºCFinal temperature = 14 ºCHow can you tell from the student’s results that the reaction is endothermic?There is a rise in temperature.Effervescence (fizzing) occurs due to the production of a gas.There is a fall in temperature.The ammonium nitrate crystals disappear and dissolve into the solution.I DON'T KNOWSUBMIT ANSWER