(c) The heat released by the reaction (d) If the acid-base neutralization produces 0.43 mole of water, what is the enthalpy change of the reaction (heat of neutralization), H, in kJ/mol?

ered You want to determine the enthalpy change for the neutralization of HCI(aq). The equipment you are allowed to use are listed below: • safety goggles tion • lab coat • protective gloves • coffee cups (2) • styrofoam lid • thermometer • scale • stirring rod • beaker 16-ml of 0.345 mol/L HCI(a) added to 42.6-ml of NaOH (aq) for a total volume which is equivalent to water (m) in the q equation a. Based on the equipment provided above, design a lab to determine the enthalpy change of neutralization of HCI(aq). Ensure you use numbered steps. When you carry out the experiment, you observe a temperature change of 3.80°C. b. Calculate the quantity of heat transferred to the calorimeter based upon the data provided. c. Based upon the data provided, calculate the molar enthalpy for the neutralization of HCI(aq). d. If the mass of volume of the HCl(aq) was increased, would the value of Q be different. Explain your reasoning. e. Provide a thorough concluding statement that includes the…

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs

How many mole is present in the reactant and product in the given belwo

Which statement about the reaction illustrated in the diagram is true? (B). (A] (C) (D) (E) O The energy required to break the bonds is more than the energy released upon forming new bonds. The energy required to break the bonds is less than the energy released upon forming new bonds. O No heat is required to start the reaction. The reaction is endothermic.

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ ((b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =  kJ(c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =   kJ(e) Calculate E when 880.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K   kJ HopHelpCh5N1

The reaction that produces the water gas mixture, described in Question 6.99, is C(s) + H₂O(g) → CO(g) + H₂(g) This reaction requires an input of 131 kJ of heat for every mole of carbon that reacts. (a) Is this reaction endothermic or exothermic? (b) What is the energy change for this reaction in units of kJ/mol of carbon?

8.2

The heat gained by the solution in  reaction two is 5.3 kJ. how many moles of NaOH were consumed ? what was the enthalpy of reaction ? (In kJ/mole)

When 3.8 g A are reacted with 8.5 g D,  according to the balanced chemical equation below, 33 kJ of energy are released.  Please calculate the enthalpy for this reaction when 3 moles of G are produced.  2A + 3D = 2Z + 3G  given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole