Enthalpy change ?? Q4 Calorimetry reactions . When 50.0 mL of 1.0 M HCI and 50.0

Question

Enthalpy change ?? Q4 Calorimetry reactions . When 50.0 mL of 1.0 M HCI and 50.0 mL of 1.0 M NaOH is mixed in a co Calorimeter, the temperature of the solution increases from 20,2 °C to 26.6 C ate the enthalpy change (AH ) of this reaction in joules and kJ. Show all work Table values Show formula and caleulation (AH) Mass of solution (g) Specific heat 4.18 J/g-C Q 5 (Hess's Law) Given two reactions: Calculate value of AH for the following reaction number 3, by using the reactions values of 1 and 2. Show all work by writing reactions again and all calculation by changing the sign if needed. If not shown points deducted. (1) 2Cu (s) + O2 (g) ? 2CuO (s) (2) 2Cu (s) + % 02 (g) Cu,0 (s) Calculate reaction 3 as shown below ?? 310 kJ ???.-169 kJ Show all calculation steps below: Cuo) V20g)L Cu OG)

Explanation / Answer

Ans 4

Moles of HCl = molarity x volume

= 1 mol/L x 50 mL x 1L/1000mL

= 0.050 mol

Mass of HCl = moles x molecular weight

= 0.050 mol x 36.5 g/mol

= 1.825 g

Moles of NaOH = molarity x volume

= 1 mol/L x 50 mL x 1L/1000mL

= 0.050 mol

Mass of NaOH = moles x molecular weight

= 0.050 mol x 40 g/mol

= 2 g

Mass of solution = 1.825 + 2 = 3.825 g

Change in temperature (T2-T1) = 26.6 - 20.2 = 6.4°C

Temperature increased during the process, it is exothermic reaction.

Change in enthalpy

H = - m x Cp x (T2-T1)

= - 3.825 g x 4.18 J/gC x 6.4 C

H = - 102.3264 J

H = - 102.3264 J x 1kJ/1000J

H = - 0.1023 kJ

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