What would be the effect on the enthalpy change determined if the temperature probe read lower than the true temperature? Explain?
(this is just asking for an overall trend, nothing that requires specific data)
What would be the effect on the enthalpy change determined if the temperature probe read lower...
1. What would be the effect on the enthalpy change determined if the temperature probe read 1.0°C lower than the true temperature? Explain. (2 pts)
The enthalpy of neutralization is −55.8 kJ/mol. What is the temperature change when 100 mL of 2 M HNO3(aq) is mixed with 100 mL of 2 M KOH(aq)? (assume density and specific heat capacity are the same as water)
29 NEUTRALİZATION CALORIMETRY 3-THERMODYNAMICS: ENTHALPY OF EXERCISES 1. If the final te or erature taken in part I was higher than the true value, the calculated value for the heat capacity of the lower than the true value? calorimeter be higher than in the process of transferring the metal cylinder from the hot water to the in part II, the cylinder lost some heat, would the calculated value 2. If for the specific heat of the metal be higher or...
If the freezing point of the solution had been incorrectly read 0.3 °C lower than the true freezing point, would the calculated molar mass of the solute have been too high or too low? Explain. Select all that apply. Select all that apply. The resulting molar mass (g/mol) would be smaller since the mol term is in the denominator. A larger ΔT results in a lower calculated molality of the solution, and thus smaller number of moles. The resulting molar...
Explain what effect the following scenarios would have on the calculated specific heat (i.e. would it be calculated artificially high, low, or have no effect). Your explanation should address what variable(s) would be affected by the scenario and how that affects the calculation of specific heat.(1.5pt each) A student accidently dropped the piece of metal on the countertop during the process of transferring it from the boiling water bath to the calorimeter, but was quickly picked up and put into...
POST LAB QUESTIONS. 1. If you used more water in your calorimeter, would the observed temperature change upon the addition of the hot solid object be larger or smaller than the temperature change you observed? Explain. 2. Your instructor handed you a 1-L sample of a liquid and asked you to determine its specific heat. How would you determine the specific heat of the liquid using the equipment in this lab? 3. What effect would not covering the calorimeter cup...
For an ideal gas, whose temperature increases from T1 to T2, what would be its enthalpy change? (a) Cv (T2-T1) (b) Cv (T1-T2) (c) Cp (T2-T1) if the heat capacities stay constant during the temperature range
7.How would the molar mass of the unknown acid be affected (higher, lower, or no change) if the follow-ing errors occurred? Briefly explain why in each case. a.The pH meter was incorrectly calibrated to read lower than the actual pH. b.During the titration, several drops of NaOH missed the reaction beaker and fell onto the bench top. c.In Part B of the procedure the acid was dissolved in 75 mL of distilled water rather than the 50 mL called for...
Given the change in temperature during the course of a reaction what formula would you use to calculate qp? In a coffee-cup calorimeter the heat absorbed by the water is equal to the heat given off by the reaction of the solutes. That is, the enthalpy of a reaction, AH is defined as the quantity of heat transferred under constant pressure, AH = -qp Given the change in temperature during the course of a reaction what formula would you use...
What effect would an incomplete decomposition of KCLO3 have on an experimentally determined molar mass? Explain using the ideal gas law