How much heat is produced by the combustion of 4.67g of magnesium (24.30 g/mol)? Mg(s) + 1/2 O2(g) → MgO(s)          ΔH = -601.6 kJ

If 0.067 mol of hydrochloric acid  (HCl)  is mixed with 0.067 mol of sodium hydroxide  (NaOH)  in a "coffee cup" calorimeter, the temperature of  5.1 g  of the resulting solution increases from 25.0 ° C to  34.0 ° C.   Given that  the energy released is    2.2  ×  101  cal when the specific heat of the resulting solution is  1.00 cal/g− ° C,  use a conversion factor to convert the energy released to joules (J). Enter your answer in scientific notation. Be sure to answer all parts.

Write and balance the equation for the complete combustion of acetylene,  C2H2.  Phase symbols and energy changes are optional.

The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03  g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of  19.9 oC, and the final temperature after addition is  26.8 oC. What is the molar enthalpy of neutralization, in units of kJ/mol? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the aluminum cup: 0.903 J g-1 oC-1. the density of the two solutions is the same as that of water: 1.00 g/mL. the heat capacity of the two solutions is the same as that of water: 4.184 J g-1 oC-1. Perform all calculations without rounding, but then provide your answer to the correct number of significant figures.

According to the following reaction, how many grams of hydrogen would be needed to produce 5.450 x 103 kJ of energy? Assume excess oxygen.  Do not type units into your answer.   H2(g) + 1/2 O2(g) ⟶⟶ H2O(l)     Δ?=−285.83??ΔH=−285.83kJ

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

5. A 1.500-g sample of a hydrocarbon is placed in a bomb calorimeter and undergoes combustion. The temperature of the calorimeter rises from 20.00°C to 23.55°C. If the calorimeter has a heat capacity of 40.3 J/°C, what is the heat of combustion (qv) for this hydrocarbon in kJ/g? 6. The heat of sublimation for iodine is 62.4 kJ/mol, at 25°C and 1.00 atm. What is AE for the sublimation of iodine (shown below) under these conditions? 2 (s) F 2 (g) volsd 7. A bomb calorimeter with heat capacity of 1.500x103 J/°C was used to study combustion of terbium (Tb) in excess oxygen: 4 Tb (s) + 3 O2 (g) →2 Tb2O3 (s) When 1.000-g of terbium was burned, a temperature increase of 3.908°C was observed. What is the AE for the reaction, in kJ/mol of Tb2O3?

In a constant-pressure calorimeter, 70.0 mL of 0.340 M Ba(OH), was added to 70.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 24.12 °C to 28.75 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g · °C.) respectively), what is AH for this reaction (per mole H, O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,O

According to the equation below, do the products have stronger or weaker bonds than the reactants? C (s) + 2H (g) → CH4 (g), ΔHrxn = -74.86 kJ/mol

In an industrial process to produce ammonia (NH3); nitrogen, N2, reacts with hydrogen, H2, the enthalpy change (∆H) is – 46 kJ/mol. Write a correctly balanced equation for this reaction. Would this reaction absorb heat or give out heat to the environment?