If 0.0244mol hydrochloric acid HCl is mixed with 0.0244mol of sodium hydroxide NaOH in a "coffee cup" calorimeter, calculate the temperature change of 90.4g of the resulting solution if the specific heat of the solution is 1.00cal·g°C and the quantity of heat released by the reaction is ×1.52103cal. Round your answer to 3 significant figures.

If you performed a similar experiment in the lab and used the following data to calculate the enthalpy of solution + neutralisation for sodium hydroxide. How many significant figures should you present your answer to? (Pay special attention to your value for temperature change, this may have fewer significant figures than you are expecting.) [1 mark]Volume HCl(aq): 40.0 mLVolume H2O: 60.0 mLMass of NaOH: 1.511 gInitial temperature: 20.5 oCFinal temperature: 29.9 oCQuestion 26Answera.3 significant figuresb.5 significant figuresc.4 significant figuresd.1 significant figuree.2 significant figures

Magnesium metal reacts with hydrochloric acid according to Reaction 1.Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)Reaction 1During an experiment to measure the molar enthalpy ΔH° of Reaction 1, a student placed 100. mL of dilute HCl(aq) into a coffee cup calorimeter, as shown in Figure 1.Figure 1  Coffee cup calorimeterAfter monitoring the solution temperature for 1 min, 0.486 g of Mg(s) was then added to the solution inside the calorimeter and stirred while continuing to monitor the temperature until the Mg(s) was completely consumed.  The results of the experiment are shown on the graph in Figure 2.Figure 2  Graph of temperature versus time during the reaction of magnesium with hydrochloric acidAccording to the first law of thermodynamics, the heat produced (or consumed) by a reaction qrxn must be equal to the heat transferred to (or taken from) the surroundings (ie, the solution and the calorimeter), as expressed by Equation 1.−qrxn = qsurroundings = qsolution + qcalorimeterEquation 1 Question 41Based on the results of the calorimetry experiment described in the passage, the magnitude of the molar enthalpy ΔH° for Reaction 1 (in kJ/mol Mg) is closest to which of the following?  (Note: Assume that the HCl(aq) has a density of 1.0 g/mL and a specific heat capacity of 4.0 J/(g∙°C), and that qcalorimeter ≈ 0.)A.8.84B.18.2C.442D.844

When 1.00g of sodium hydroxide is dissolved in 100.0 g of water in an insulatedcontainer the temperature rises from 20.00°C to 22.66°C. Calculate the enthalpychange for the solution. State any assumptions made.NOTE: Dissolving reactions due not have limiting reagents.

A student dissolves 11.6 g of sodium hydroxide NaOHin 300. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 23.0 °C to 33.9 °C over the course of 6.1 minutes.Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction:→NaOHs + Na+aq  OH−aqYou 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 NaOH. kJmol

When 100 cm3 of 1.0 moldm−3 HCl is mixed with 100 cm3 of 1.0 moldm−3 NaOH, the temperature of the resulting solution increases by 5.0 °C. What will be the temperature change, in °C, when 50 cm3 of these two solutions are mixed?A.     2.5B.     5.0C.     10D.     20