A solid 30.2 cm^3 block of KClO3 is heated in the laboratory and decomposes according to the following reaction. What is the change in enthalpy in kj when all the solid KClO3 decomposes? The density of KClO3 is 2.34 g/cm^3. 2KClO3(s)-> 2KCl(a)+3O2(g)=-89.4kj

After a few minutes on the hot plate some sodium bicarbonate (NaHCO3) begins to decompose into sodium carbonate, CO₂(g) and H₂O(g). Using standard enthalpies of formation, calculate the enthalpy change for this reaction. Use the following data. The standard enthalpy of formation for NaHCO3 is -997 KJ/Mol and sodium carbonate is -468 KJ/Mol.

nuraipy changes in chemical reactions Read through pages 18-20 in your laboratory manual for information on how to calculate the enthalpy change in a solution. Part A - Calculating ms In a calorimetry experiment 5.6 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 °C. The effective mass of the glass in the thermos flask (mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-¹K-1¹. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-¹K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Calculate the total mass of solution in kilograms (ms) Give your answer to four significant figures. ▾ View Available Hint(s) Hint 1. Calculating ms mg = mass water (kg) + mass solute (kg) —| ΑΣΦ Submit Request Answer ? kg < Pear 10

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

A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH)3(s)→Al,03(s) + 3 H,0(1) AH=41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 2 Al,0, (s) + H,0(1) Al(OH), (s) kJ 3 3 Al, O, (s) + 3H,0(1) → 2A1(OH), (s) kJ 3 Al(OH), (s) → Al, 0, (s) + H,0() |kJ 3

In a coffee-cup calorimeter, 100.0 mL of 1.1 M    NaOH and 100.0 mL of 1.1 M   HCI are mixed. Both solutions were originally at 22.8°C. After the reaction, the final temperature is 30.2°C. Assuming that all the solutions have a density of 1.0 g/cm^3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCI  by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH = ---------  kJ/mol

Given the following reactions Fe203 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g) AH = -28.0 kJ 3Fe (s) + 4CO2(s) → 4CO (g) + Fe304(s) AH = +12.5 kJ the enthalpy of the reaction of Fe203 with CO 3F2203 (s) + CO (g) – CO2 (g) + 2FE304 (s) 1s kJ. O- 59.0 O 40.5 O -15.5 O 109

What is the enthalpy change for the reaction MgO(s) + 2HCl(g) →MgCl2(s) + H2O(l)? Enthalpies of formation are −601.7 kJ/mole for MgO, −92.3 kJ/mole for HCl, −641.6 kJ/mole for MgCl2, and −285.8 kJ/mole for H2O(l).

If a reaction causes 25.0 g of water to decrease temperature by 14.24 oC at constant pressure, what is the change in enthalpy for the reaction in kJ ? (The specific heat capacity of water is 4.184 J/g oC). Assume no heat transferred to surroundings.