Volume of HCL=50 Molarity HCL = 2.199 Volume of NaOH = 54 Molarity of NaOH= 2 In
ID: 794031 • Letter: V
Question
Volume of HCL=50 Molarity HCL = 2.199 Volume of NaOH = 54 Molarity of NaOH= 2 Initial temperature of HCL = 23C Initial temperature of NaOH= 23.2C 1). Total mass of the final solution by adding he mass of initial HCL solution (density of 2M HCL is 1.03g/mL), the mass of water (density of water is 1.00g/mL), and the mass of magnesium. 2) Heat required to raise the MgCl2 solution to the maximum temperature assuming that the heat capacity of your final MgCl2 solution is 3.97 J/gC 3). Heat required to raise the calorimeter to the maximum temperature using the value for the heat capacity of 6.26 J/C 4) Total heat evolved by the reaction by adding the heats required to raise both the solution and the calorimeter to the maximum temperature. 5). Heat evolved per mole of Mg 6) Change in enthalpy for the following specific reaction. Be sure to indicate the correct sign (- or +) for the change in enthalpy. Mg(s) + 2H(aq)===>Mg(aq)+H2(g)Explanation / Answer
miilimoles of HCL = 50*2.199 =109.95
millimoles of Mg = 0.4045/24.3 =16.646
in balanced equation ratio of mg : HCL = 1:2
so Mgcl2 formed = 16.646 millimoles
HCL left = 76.657
H2 formed = 16.646 millimoles
1)Total MAss = (density of hcl * volume ) + Mg mass + water mass
= ( 1.03 g/ml x 50 ml) +(0.4045)+(1*50)
= 101.90 grams of solution
2) You did't provide final temp .....so i assumed it as 41.9 degrees
Q = Mass of Mgcl2 * C * delta T
Q = (0.016646*95.2) (3.97 )(41.9-23)
= 118.5761 J
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3) remember heat capacity is defined as heat required to raise the temperature by 1 degree so
for 1 degrre raise you need 6.26 J
So form max temperature
heat should be =6.26 * 18.9 = 118.314 J
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4)
Total heat = 118.314 + 118.5761
= 236.890 J J
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5)
heat evolved per mole Mg =
= 236.890/0.01664
= 14270 .491 J
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6)
Delta H = - 142.491 <----answer
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