7
a)
The balanced reaction is
The enthalpy change of the reaction is -1204 kJ/mol. Since it is negative, by convention it means energy is released.
Hence, energy released when 1 mole of MgO is formed is 1204 kJ.
Hence, when the energy released is 395 kJ, the number of moles of MgO that must have formed is
Molecular mass of MgO is 40.30 g/mol.
Hence, mass of MgO formed is
b)
Note that the energy of product is lower than the energy of reactants. Hence, the enthalpy change is negative for this exothermic reaction.
7.) Given the following reaction: 2 Mg (s)+ O2 (g) 2 MgO (s) AH 1204 kJ/mol...
For the balanced thermochemical equation below: 2 Mg(s) + O2(8) + 2Mg0g AH (MgO) --601.8 Assuming 40.0 g of oxygen gas is consumed in the presence of an excess amount of magnesium, how much heat in kJ is evolved (sign is assumed to be negative for heat evolved; do not include the sign). Report to the nearest 0.1 kJ.
What is the change in enthalpy in kilojoules when 2.30 mol of Mg is completely reacted according to the following reaction 2 Mg(s) + O2(g) – 2 MgO(S) AH = -1204 kJ STARTING AMOUNT ADD FACTOR ANSWER RESET () -0 o 0.001 2 -1204 1000 24.31 2770 -2770 2.30 2.30 6.022 * 10 32.00 32.00 -5540 -5540 40.31 40.31 -1380 -1380 1380 1380 5540 kJ gmg mol Mgg MgO gomol Mgo m olo:
Question 21 4 pts Consider the following reaction: 2 Mg + O2 → 2 MgO AH rxn=-1203 kJ Calculate the amount of heat (in kJ) associated with complete reaction of 4 moles of Mg. 0-2406 kJ 0-601.5 kJ O-1203 kJ O-4812 kJ none of the above
2Mg(s) + O2(9) --> 2Mgº(s) molar mass Mg = 24.30 g/mol molar masso2 = 31.98 g/mol molar mass Mgo = 40.29 g/mol If 12.6 grams of magnesium completely react to form magnesium oxide according to the equation given, how much magnesium oxide is produced?
Hrnx MG Hrnx MgO Trial 1 -1356.2 kJ/mol -645.33 kJ/mol Trial 2 -1543.9 kJ/mol -650.62 kJ/mol Trial 3 -1540.2kJ/mol -655.23 kJ/mol experiment 9 Post-lab Questions is advised that you wait until next week to submit your results and post-lab questions due to the challenging nature of them. Mess's law is all about utilizing a series of reactions and their AH to determine the AH of an unknown reaction. AH=2829 Mgw + 2HC1,09) -> MgCl2log + H2lo AH = ???? MgO...
Specific heat = 4.18 J/g*C MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of MgO(s) to 45.0 mL HCI@ 22.0'C. The temp of the calorimeter rose to 23.5°C. What is qarin kJ? What is the AH in kJ/mol of Mgo for this reaction? Density HCI = 1.05 g/mL
Consider the following reaction: 2Mg(s)+O2(g)→2MgO(s)ΔH=−1204kJ a. How many grams of MgO are produced during an enthalpy change of -95.0 kJ ? b. How many kilojoules of heat are absorbed when 7.60 g of MgO(s) is decomposed into Mg(s) and O2(g) at constant pressure?
What is the mole of magnesium, ?️H per mol of MgO, ?️H per 1 mole Mg? Part 2: Hydrochloric Acid + Magnesium The strategy for these calculations are similar to those in Part 1. In Part 2, magnesium reagent. Calculations Sheet Thermochemistry 2 II. In Part 2, magnesium is the limiting Volume of hydrochloric acid solution Density of hydrochloric acid solution 75.0 mL Mass of hydrochloric acid solution (d-m/V) Specific heat capacity of hydrochloric acid solution Change in temperature for...
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: (0.25 pt.) Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol,...
Draw a reaction-energy diagram (energy in kJ/mol) for the last step of a free radical substitution mechanism. Label correctly the: - axis (with units of measures, if applicable); - energy levels of reactants, products, transition states and intermediates (if applicable); - activation energy (or energies, if applicable); - heat of reaction (including its sign).