During an experiment, a student adds 2.90 g of CaO to 400.0 mL of 1.500 M HCl. The student observes a temperature increase of 6.00 °C. Assuming the solutionand#92;'s final volume is 400.0 mL, the density if 1.00 g/mL, and the heat capacity is 4.184 J/(g·°C), calculate the heat of the reaction, ΔHrxn.
CaO(s) 2H (aq) -----andgt; Ca2 (aq) H2(g)
During an experiment, a student adds 2.90 g of CaO to 400.0 mL of 1.500 M HCl.?
2016-03-28 4:38 pm
回答 (1)
2016-03-28 4:50 pm
Heat released from the reaction
= m c ΔT
= (400 × 1) × 4.184 × 6.00
= 10040 J
= 10.40 kJ
Molar mass of CaO = 40.08 + 16.00 = 56.08 g/mol
Number of moles of CaO used = 2.90/56.08 = 0.05171 mol
As heat is released, the reaction is exothermic.
Heat of reaction = -10.40/0.05171 = -201 kJ
= m c ΔT
= (400 × 1) × 4.184 × 6.00
= 10040 J
= 10.40 kJ
Molar mass of CaO = 40.08 + 16.00 = 56.08 g/mol
Number of moles of CaO used = 2.90/56.08 = 0.05171 mol
As heat is released, the reaction is exothermic.
Heat of reaction = -10.40/0.05171 = -201 kJ
收錄日期: 2021-05-01 13:08:44
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