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escojo2508
22.04.2020 •
Chemistry
Suppose you place 0.0600 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCl. The reaction that occurs is Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) The temperature of the solution increases from 23.08 °C (296.23 K) to 25.78 °C (298.93 K). What is the enthalpy change for the reaction per mole of Mg? Assume a specific heat capacity of the solution is 4.20 J/g∙K and the density of the HCl solution is 1.00 g/mL. 459.55 kJ/mol Show ApproachHide Tutor Steps TUTOR STEP What is the heat released by the reaction, qr? qr + qsolution = 0 qsolution = 1130 J
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Ответ:
ΔH = -459.1 kJ/mol
Explanation:
Step 1: Data given
Mass of the magnesium chips = 0.0600 grams
Volume of a 1.00 M HCL = 100.0 mL= 0.100 L
The temperature of the solution increases from 23.08 °C (296.23 K) to 25.78 °C (298.93 K)
The specific heat capacity of the solution is 4.20 J/g∙K
density of the HCl solution is 1.00 g/mL
Step 2: The balanced equation
Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq)
Step 3: Calculate heat
Q = m*C*ΔT
⇒with Q = the heat transfer = TO BE DETERMINED
⇒with m = the mass 100 mL * 1g/mL = 100 grams
⇒with C = the specific heat capacity of the solution is 4.20 J/g*K
⇒with ΔT = the change of temperature = T2 - T1 = 298.93 - 296.23 = 2.7 K
Q = 100 * 4.20 * 2.7
Q = 1134 J
Step 4: Calculate moles Mg
Moles Mg = mass Mg / molar mass Mg
Moles Mg = 0.0600 grams / 24.305 g/mol
Moles Mg = 0.00247 moles
Step 5: Calculate the enthalpy change for the reaction per mole of Mg
ΔH = -1134 J / 0.00247 moles
ΔH = -459109 J/mol = -459.1 kJ/mol
(negative since it's an exothermic reaction)
Ответ: