Since temperature of the solution rises in both the cases, both reactions are exothermic in nature and ∆H is negative.
[References] INTERACTIVE EXAMPLE Using a Coffee-Cup Calorimeter Suppose you place 0.0500 g of magnesium chips in...
Suppose you place 0.0600 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCl. The reaction that occurs is Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) The temperature of the solution increases from 23.11 °C (296.26 K) to 25.81 °C (298.96 K). What is the enthalpy change for the reaction per mole of Mg? Assume a specific heat capacity of the solution is 4.20 J/g∙K and the density of the HCl solution...
You mix 125 mL of 0.270 M CsOH with 50.0 mL of 0.675 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 20.70 °C before mixing to 23.82 °C after the reaction. CsOH (aq) + HF (aq) ---> CsF (aq) + H2O (l) What is the enthalpy of reaction per mole of CsOH ? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g...
You mix 125 mL of 0.180 M CsOH with 50.0 mL of 0.450 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.30 °C before mixing to 23.38 °C after the reaction. CsOH(a) +HF(a)-CaF a)+H20() What is the enthalpy of reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 Jg K. Enthalpy of reaction- siol
You mix 142 mL of 0.254 M CSOH with 130.0 mL of 0.2774 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 20.10°C before mixing, to 22.90°C after the reaction. CsOH (aq) + HF (aq) --> CsF (aq) + H20 (1) What is the heat [g] for this reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions are 4.18 J/(g.K). 90.5...
You mix 2.58 mL of 0.613 M CsOH with 510.0 mL of 0.3101 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 20.50 degree C before mixing, to 23.50 degree C after the reaction. CsOH (aq) + HF (aq) rightarrow CsF (aq) + H_2O (l) What is the heat [q] for this reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions...
In a coffee cup calorimeter, 100.0 mL of 1.00 M NaOH and 200.0 mL of 0.80 M HCl are mixed at 25.0oC. After the reaction, the temperature is 29.5 oC. Assuming all solutions have a density of 1.00 g/cm3 and a specific heat capacity of 4.18 J/oC g, what is the enthalpy change (kJ) for the balanced reaction? HCl(aq) + NaOH(aq) => NaCl(aq) + H2O(l)
Coffee Cup Calorimetry: Specific Heat [Review Topics) (References] Use the References to access important values if needed for this question, progress In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy change of a solution phase reaction A student heats 61.07 g tin to 97.98 °C and carefully lowers it into a cup containing 82.04 g water at 20.93 °C. She measures...
You mix 176 mL of 0.310 M CsOH with 76 mL of 0.6458 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 35.9 C degree before mixing, to 43.8 C degree after the reaction. CsOH (aq) + HF (aq) arrow CsF (aq) + H2O (l) What is the heat [q] for this reaction per mole of CsOH? Assue the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions...
In a coffee-cup calorimeter, 50.0 ml of .100 M AgNO3 and 50.0 ml of .100 M HCl are mixed to yield the following reaction: Ag+(aq) + Cl-(aq) --> AgCl(s) The two solutions were initially at 22.6°C and the final temp is 23.4°C. Assume that the final solution has a mass of 10.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate delta for the reaction in kJ/mole of AgCl formed.
Question #5: PART A: In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 ∘C. If 8.90 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution ΔHsoln of CaCl2 is −82.8 kJ/mol. QUESTION #8: PART A: A calorimeter contains 18.0 mL of water at 12.0 ∘C . When 2.50 g of X (a...