Part D . answer trial 1 and trial 2 for #2 & #3 Part E. Answer all the blank spo

Question

Part D . answer trial 1 and trial 2 for #2 & #3 Part E. Answer all the blank spots part F. Answer trail 1 and 2 for #1,#2,#4,#5 For my chemistry lab calculations Experiment 13 A Carbonate Analysis; Molar Volume of Carbon Dioxide The reoction of hydrochloric ocid on calcium carbonote produces carbon dioxide gas . To determine the percent calcium carbonate in a heterogeneous misture . To determine the molar volume of carbon dioxide gas at 273 K and OBJECTIVES 760 torr oheetines in dWerent phoses The following techniques are used in the Experimental Procedure TECHNIQUES Calcium carbonate is perhaps the most prevalent simple inorganic compound in Earth's crust. More commonly known as fimestone, calcium carbonate is found in many forms and formulations. Calk·marble (a dense form of calcium carbonate), shells of shell- fish, stalactites, stalagmites (Figure 13.1), caliche, and the minerals responsible for hard INTRODUCTION water have their origin from fossilized remains of marine life. In this experiment, the percent by mass of a carbonate salt in a heterogeneous mix- ture is determined. Your instructor may choose anhydrous calcium carbonate, anhy- carbonate, or potassium carbonate as the salt. For each of the carbonates, the sam¢ chemistry and analysis applies. The focus of this experiment is on calcium drous sodium carbonate. Calcium carbonate readily reacts in an acidic medium to peoduce carbon dioxide gas The calcium carbonate of the sample is treated with an excess of hydrochloric acid, and the carbon dioxide gas is collected over water. The mass, volume, and moles measured and calculated. From the stoi- chiometry of equation 13.1, the moles and mass of CaCO, in the sample are cakculated of carbon dioxide generated in the reaction are Because carbon dioxide is relatively soluble in water, the water over which the Co, is Figure 13.1 Stologmiles and collected is pretreated to saturate it with carbon dioxkle. stalacttes are primarily calcium In addition to analyzing the unknown mixture for percent calcium carbonate, the molar volume of carbon dioxide is also determined. At standard temperature and ccupied by pressure (STP), one mole of an ideal gas occupies 22.4 L: that is, its molar volume is Molor volume 22.4 L at STP. Because carbon dioxide is not an ideal gas, we may expect its molar molecuviesl of aos at o volume to vary slightly from this number in this experiment one mole 6 023 × 104 okres or tempercfure and pressure conditions Standand mperature and To make these two determinations in the experiment, two important measure- and its volume ments are made: (1) The CO, gas evolved from the reaction is collected is tion, is also measured. amouphere reac 760 o) is measured, and (2) the mass difference of the CaCO, mixture, before and after reas. Experiment 13 181

Explanation / Answer

I'm gonna help you with the part C and D, because part E and F are not in there. Put it in another question thread and I'll gladly answer it for you.

C. The volume of gass collected is simply substract the final buret reading and the innitial buret reading. The final reading was in both trials 0 mL, so the volume of CO2 collected was 39 mL for trial 1 and 20 mL for trial 2.

for the part 7 of here, you just need to substract the pressure of water with the pressure of the barometer:
for trial 1: P¨= 770-25.2 = 744.8 Torr
For trial 2: P = 770-30 = 740 Torr

D. The mass of generator loss you can calculate by substracting the innitial with the final:
Trial 1: 195.17 - 194.97 = 0.2 g
Trial 2: 195.6 - 195.4 = -0.2 g or simply 0.2 g

to get the moles, use the mass evolved:
moles CO2 = 0.2 / (12+32) = 0.0045 moles

Hope this helps

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