Step 1: Gather materials and necessary information. a) You will be provided with these initial materials:  2 plastic resealable bags  3–5 “000” size empty gelatin capsules  One 10 mL graduated cylinder to measure purified or distilled water  5 mL distilled water  1 g calcium chloride  1 Fahrenheit or Celsius thermometer  1 funnel  Clock or stopwatch b) Make sure you use the materials given only for reference purposes in Steps 1 and 2 to help you with ideas in the design phase. Building the device does not occur at this point and any materials you alter or destroy will not be replaced. c) Be sure to organize your materials and make sure that the chemicals are handled safely. d) Do not allow substances to mix until the testing phase begins. e) Be sure you have paper and a pen or pencil to record data before, during, and after the testing phase of the project. This data will be reported in your final report. f) The reaction that will be used is the dissolving of calcium chloride in distilled or purified water. The action of dissolving calcium chloride is an exothermic process that can be detected by an increase in temperature. g) Remember to treat tools and materials with care and respect, and to use all safety precautions that you would in a laboratory exercise. Step 2: Design the device. a) Begin by writing a description and/or drawing a diagram of the expected design of your device, using these requirements:  Your device must allow temperature data to be collected both before and after the device is activated.  Your device must release energy to the environment and it must be a controlled reaction. This means that you must have a way to start the reaction at a set time. Your device must maintain the room temperature for 15 seconds or more, then be activated by you to increase

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer

it is the most commonly accepted one

the missing options are :

(1) lower boiling point and a lower freezing point(2) lower boiling point and a higher freezing point(3) higher boiling point and a lower freezing point(4) higher boiling point and a higher freezing point

answer : the correct answer is option (3) higher boiling point and a lower freezing point

explanation :

when a non volatile solute is added to a solvent like water, it results in elevation of boiling point.

let us find the increase in boiling point of water when cacl₂ is added to water to make a solution of 1 m

step 1 : find molality of the solution

let us assume we have 1 l of solution.

let us convert this to grams of cacl₂.

molar mass of cacl2 is 111 g/mol

grams of cacl₂ =

mass of solute = 111 g

assuming density of solution same as water which is 1g/ml we have ,

mass of solution = density * volume

mass of solution =

mass of solution = mass of solvent + mass of solute

mass of solute = 1000g - 111g

mass of solute 889 g = 0.889 kg

the molality of the solution can be calculated as

molality = 1.12 m

step 2 : find boiling point elevation.

the elevation in boiling point is calculated as

here δtb = boiling point elevation

i = vant hoff factor which is the number of ions formed by the solute .

cacl₂ dissociates as

it forms 3 ions . therefore,

i = 3

m = molality which is 1.12 m

kb is constant for a given solvent. for water it is 0.512

the boiling point of water increases by 1.7 °c

step 3: find freezing point depression.

when a non volatile solute is added to water, it results in decrease in freezing point.

the formula to find freezing point depression is

kf is constant for water and its value is 1.86

the freezing point of water decreases by 6.2 °c

therefore we can say that, the solution will have a higher boiling point and a lower freezing point