75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC.   Then the reaction is proceeded and the final temperature is reached to 28.000 oC.  Calculate the heat of reaction in kJ / mole. Hint: Treat this mixture as a diluted solution. CP of H2O(l) = 4.184 J / g oC D of H2O = 0.988 g/ mL.

PLease help me with this. DO both please as they are calculate together but they are different questions

Use the References to access important values if needed for this question. Consider the reaction: C(s) + 1/20₂(g) → CO(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: C(s) + O2(g) CO₂(g) K₁ CO(g) + 1/2O₂(g) = CO2 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K =

When we discussed LeChatelier's Principle, we discussed the concept of supersaturated solutions. A supersaturated solution is prepared when sodium acetate is dissolved in hot water at around 80 deg C, and then the solution is cooled to room temperature.  Since no precipitation occurs, the solution is supersaturated.  The reaction is: heat + sodium acetate (s) + H2O (liq) <---> sodium acetate (aq). If you disturb the supersaturated solution of sodium acetate, which of the following statements is true? b.  Solid sodium acetate will precipitate if there is enough water present.   c.  Solid sodium acetate will precipitate if there is not too much water present.   d.  Nothing will happen.  The system is at equilibrium.   e.  Solid sodium acetate will precipitate and the solution will get warm.

BaCl, · H,O(s) loses water when it is heated in an oven: BaCl, · H,O(s) = BaCl, (s) + H,O(g) AH° = 63.11 kJ/mol at 25 °C AS +148 J/(K · mol) at 25 °C Write the equilibrium constant for this reaction. Find the vapor pressure of H,O (PH,0) above BaCl, · H,O(s) at 298 K. PH,0 bar = If AH° and AS° are not temperature dependent (a poor assumption), estimate the temperature at which PH,0 above BaCl, · H, O(s) will be 1 bar. T = °C

1 atm = 760 mm Hg R = 0.0821 L atm/ mol K K = °C + 273 PV = nRT Molar volume @ STP, 1 mole = 22.4L of ideal gas 1. produce nitrogen gas. One important reaction is listed below The inflation of an automobile airbag involves several chemical reactions that 10NA(s) + 2KNO3(s) –> K2O(s) + 5Na2O(s) + N2(g) If a side airbag contains 71.3 g Na and 75.9 g KNO3, to what pressure, in mm Hg, would a 5.30 L airbag inflate (due to the production of nitrogen gas) if the reaction occurs at a temperature of 72.0°C.

3.02 g of sodium sulfate was mixed into a solution containing 48.5 mL of 0.185 mol/L aqueous silver nitrate:   Calculate the maximum mass (in g) of precipitate that can form.   Note: Balanced chemical eq. with state of each compound required.       2. What is the molar concentration of sodium ions in the resulting solution?

2. According to Le Chatelier's principle, it indicates where the balance is favored (Reactants or products) of the following unbalanced reaction H₂O(a) + Fe(s) + H₂(g) + Fe3O4(s) + Heat Write your answer on the line a) Decreases ia [H2): b) The temperature of the system decreases: c) The system pressure increases:

Calculate ArH for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given >ArH"s Ca(s)+CO2(g)+1/202(g) →CaCO3(s), ArH= -812.8 kJmol-1 2Ca(s)+02(g) →2CaO(s), ArH= -1269.8 kJmol-1 ArH=-177.9 kJ mol-1 ArH= 177.9 kJmol-1 ArH=327.9 kJmol-1 ArH=-327.9 kJmol-1

The equilibrium constant for the acid ionization of mercaptoethanol (HSCH2CH2OH) is HSCH2CH2OH(aq) = H+(aq) + SCH2CH2OH-(aq)               k= 1.91 x 10-10 Which of the following is/are true regarding this equilibrium? And why? 1. The reaction is product-favored. 2. The reaction is reactant-favored. 3. Equilibrium lies far to the right. 4. Equilibrium lies far to the left.