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Calcium carbonate, CaCO3, decomposes upon heating according to the following equation.
CaCO3 (s) ∆ CaO (s) + CO2 (g)
0.20 mol of CaCO3 is heated in a 2.0 L vessel. After heating, it is found that the pressure of
the gas is 44.08 kPa at 30°C.
i) Determine the number of moles of gas formed from the decomposition of CaCO3 .
ii) The mass of CaCO3 left after the reaction was completed
iii) The partial pressure of hydrogen gas in the vessel when 0.10 mol of hydrogen gas is added
to the vessel at the same temperature.
Answers: 3
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Vi limitens. vastery test select the correct answer. which statement explains why large atoms are more reactive than small atoms? a. large atoms have valence electrons farther from the nucleus and lose them more readily. b. large atoms have greater ionization energy, which they can utilize during a reaction. c. large atoms have a greater number of electrons that they can lose during a reaction. d. large atoms have more energy levels, so they have more energy to pass on in a reaction. reset next
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The sum of the oxidation numbers in a neutral compound is always
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An unknown insoluble substance displaced the water shown. it's mass is indicated on the triple beam balance. mass = a. 694 b. 693.5 c. 693.0 d.693.8
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Calcium carbonate, CaCO3, decomposes upon heating according to the following equation.
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