To find the delta H for the reaction, we can use the formula q = mcΔT, where q is the heat absorbed or released, m is the mass of the solution, c is the specific heat, and ΔT is the change in temperature.įirst, we need to find the mass of the solution: (a) the reaction of aqueous solutions of silver nitrate and sodium iodide (b) the. Molarity of AgNO3 = moles of AgNO3 remaining / total volume of solution = 0.554 mmol / (12.0 mL + 21.22 mL) = 0.017 M The net ionic equation for the reaction of cobalt(II) chloride and. Moles of AgNO3 remaining = moles of AgNO3 - (3 * moles of CoCl3) = 2.4 mmol - (3 * 1.846 mmol) = 0.554 mmol To find the molarity of the excess reactant after the reaction completes, we first need to find the moles of AgNO3 remaining: Now, we can find the mass of the precipitate: Now, we can find the moles of Co(NO3)3 formed: Since we have more than 3 times the moles of AgNO3, CoCl3 is the limiting reactant. The stoichiometry of the reaction is 3:1, so we need 3 times more moles of AgNO3 than CoCl3. We can do this by comparing the moles of each reactant: To find the mass of the precipitate, we first need to determine the limiting reactant. The net ionic equation is obtained by canceling out the spectator ions (NO3- and Cl-):ģAg+ (aq) + Co3+ (aq) = Co3+ (aq) + 3Ag+ (aq) Now, we can write the net ionic equation by breaking down the aqueous compounds into their respective ions:ģAg+ (aq) + 3NO3- (aq) + Co3+ (aq) + 3Cl- (aq) = Co3+ (aq) + 3NO3- (aq) + 3Ag+ (aq) + 3Cl- (aq) The balanced molecular equation is already given:ģAgNO3 (aq) + CoCl3 (aq) = Co(NO3)3 (s) + 3AgCl (aq) First, we need to write the balanced molecular equation and then the net ionic equation.
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