QUESTION 9 Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂2(1)→ 2 H₂O(l) + O₂(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pres -0.0217 kJ -2.31 × 104 kJ -23.1 kJ O-11.5 kJ 1.44 kJ

For the reaction below, ΔHrxn = −126 kJ/mol. How much heat is released when 2.00 mol of NaOH is formed in the reaction?2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)

Calculate the quantity of energy transferred (q), in kJ, by the combustion of 177 mL of acetone (C3H6O)? C3H6O(l) + 4 O2(g) → 3 CO2(l) + 3 H2O(g)        ΔHrxn = -1790 kJ Given: The density of acetone is 0.788 g/mL and its molar mass is 58.08 g/mol IMPORTANT: Enter both the sign and the value (no units), using 3 significant figures.

How much energy is required to produce 11 grams of glucose (C6H12O6; 180 g/mol) from CO2 and H2O. Use the following combustion equation to help you answer the question? C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)  ΔH=−2900kJ

How much heat (in kJ) will be released (AH) if 1.20 mol of SrO is mixed with 0.951 mol of CO2 in the following chemical reaction? Sro (s) + CO2 (g) → SrCO3 (s) AH° = -234 kJ/mol

In the following reaction, how much heat is generated when 3.21 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol

Part O Which reactions are exothermic?   Reaction 1: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) + 2220 kJ   Reaction 2: 4 H2(g) + 2 O2(g) → 4 H2O(l) + 1140 kJ   Reaction 3: 2 H2O(l) + 88 kJ → 2 H2(g) + O2(g)   Reaction 3 Reactions 2 and 3 Reaction 1 and 2 All reactions are since they produce products.

A chemist measures the enthalpy change ΔH during the following reaction:

In a coffee cup calorimeter, 50.0 mL of 0.130 M AGNO, and 50.0 mL of 0.130M HBr are mixed. The following reaction occurs. Ag*(aq) + Br¯(aq) → AgBr(s) If the two solutions are initially at 23.51°C, and if the final temperature is 24.82°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J°C¯1g=1. 84.2 X kJ/mol

The following chemical reaction is exothermic releasing 283 KJ/mole of heat.  CO(g) + ½O2(g) ⟷ CO2(g) How would you increase the amount of product produced from this reaction?