Mol of MgO is = 0.0124 mol
delta H = - 140.32 kJ/mol
Calculation is given in the image.
Input Data Reactant Mass (9) .5000 1.00 Mg Volume (mL) 100.0 100.0 AT (C") 19.7 Mgo 9.0 Calculated Enthalpies of Reaction Mg(s) + 2 HCl(aq) --> MgCl2(aq) + H2(g) AH = -95.76 kcal/mol MgO(s) + 2 HCl(aq) --> MgCl2(aq) + H2O(1) AH = -36.27 kcal/mol Problem: Solve for the following enthalpy changes 1) When 6.73 g NaOH(s) is reacted with 200.0 mL of HCl(aq), the temperature increases 20.10 Celsius degrees NaOH(s) + H"(aq) --> Na"(aq) H2O(0) AH = ? 2)...
help me solve 1-3 Input Data Reactant Mg MgO Mass (9) 2300 104 Volume (mL) 100.0 1000 AT (C) 10.4 9.6 Calculated Enthalpies of Reaction Mg(s) + 2 HCl(aq) --> MgCl, (aq) + H29) AH = -459.83 kJ/mol MgO(s) + 2 HCl(aq) -> MgCl2(aq) + H20(0) AH = -155.66 kJ/mol Mg(s) + 4029) -> Mg(s) AH = -589.99 kJ/mol Problem: Solve for the following enthalpy changes 1) When 6.07 g NaOH(s) is reacted with 200.0 mL 0.759 M HCl(aq), the...
Magnesium Ribbon Record all masses to the 0.01 g, except for the mass of Mg and the mass of MgO used. These should be recorded to the 0.0001 g. Table 7 Mass (g) 40 28.54 Calorimeter Calorimeter & Water & Acid 4.9 103.66 Water & Acid 4075.12 Magnesium Ribbon 490.1212 Enter the following temperatures to the nearest 0.1°C. Table 8 Temperature (°C) Calorimeter & Acidic Water 49 19.5 Maximum Temperature Reached 49 25.2 V Magnesium Oxide Table 9 Mass (g)...
Consider the following reaction: 2 HCl(aq) + 1 Mg(s) → 1 MgCl2(aq) + 1 H2(g) ΔH°rx = -465.8 kJ Determine the amount of heat released, in kJ, of each of the following scenarios. Give each answer to 2 decimal places. (a) 10.69 g of Mg(s) is reacted with excess HCl(aq)· (c) 1.17 g of H2(g) is produced from the reaction after completion. (b) Excess Mg(s) is added to 440 mL of 0.996 M of HCl(aq)· (d) 580 mL of a...
Please help fill in data table and answer questions. thank you! Date DATA Reaction 1 (Mgo) Reaction 2 (Mg) T. Volume of 1.00 M HCI 2. Final temperature, t 3. Initial temperature, t 50.0 m 50.0 mL Bc -C 20.8 C 4. Change in temperature, t 5. Mass of solid 6. Heat, q 7. ΔΗ 8. Moles mol Mgo mol Mg kJ/mol kJ/mol 10. Determine ΔH/mol Mg for reaction (4)" (10.) 11. Percent error Outside of lab, you must print...
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,...
Consider the following reaction: Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g) ΔHrxn = –4.6 × 102 kJ a. Is this reaction endothermic or exothermic? Circle one. [1] b. How much heat is evolved when 1.37 g of Mg are dissolved in excess HCl? [5] c. If 1.37 g of Mg are dissolved in enough HCl to make 250.0 mL of solution in a coffee-cup calorimeter, what is the final temperature of the solution? (Assume density...
6. Metallic Mg reacts with hydrochloric acid according to the following equation: Mg(s) + 2 HCl (aq) → MgCl2 (aq) + H2(g) The enthalpy change associated with this reaction can be determined with an ice calorimeter. If 14.71 g of ice are melted when 0.2649 g of Mg reacts with excess hydrochloric acid, what is AH (in kJ/mol Mg) for the reaction written above? The heat of fusion of ice is 333 J/g.
a) 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: Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol, calculate the percent error
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