When 50.0 mL of 2.00 M HCI is mixed with 50.0 mL of 2.00 M NaOH at 24.5°C, the solution temperature increases to 50.3°C. Calculate the AHpxn in kJ/mol HCl? Assume the density of the solution is 1.00g/mL, Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. Report your answer to 3 sf and remember to use the correct sign for AHn- %3D Your Answer: Answer units

When 50.0 mL of 2.00 M HCI is mixed with 50.0 mL of 2.00 M NaOH at 24.5°C, the solution temperature increases to 50.3°C. Calculate the AHpxn in kJ/mol HCl? Assume the density of the solution is 1.00g/mL, Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. Report your answer to 3 sf and remember to use the correct sign for AHn- %3D Your Answer: Answer units

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the total enthalpy change (kJ) for the following reaction: H2O (s, 90 g, –10. oC) --> H2O (l, 90 g, 10. oC) (The specific heat capacity of ice is 2.0 J/g×oC; the specific heat capacity of liquid water is 4.2 J/g×oC; the enthalpy of fusion for H2O at 0 oC is 6.0 kJ/mol.)
Macmillan Learning In a constant-pressure calorimeter, 55.0 mL of 0.330 M Ba(OH), was added to 55.0 mL of 0.660 M HCI. The reaction caused the temperature of the solution to rise from 24.25 °C to 28.75 °C. If the solution has the same density and specific heat as water (1.00 g/mL. and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H₂O
Consider the following chemical equation for which the enthalpy of reaction equals +26.9 kJ. 2 ICI(g) 12(g) + Cl2(g) At 25 °C, Kp = 5.0 x 10-6. If the temperature is increased to 35.0 °C, what changes (if any) will be observed? O a. Kp will remain unchanged. O b. Kp will increase. O c. [12] will decrease. O d. Kp will decrease. O e. [ICI] will increase.
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ab The enthalpy of solution (AH) of NaNO3 is 20.4 kJ/mol. If 8.50 g NaNO3 is dissolved in enough water to make a 100.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g °C and the density of the solution is 1.02 g/mL). Tap here or pull up for additional resources 1 Q @ 2 W # 3 E $ 4 R % 5 T Question 1 of 10 6 Y & 7 U 8 1 9 1 4 7 +/- 0
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In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
A student dissolves 11.0 g of sodium hydroxide (NaOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 21.0°C to 31.1 °C over the course of 6.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. - Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy A/, per mole of NaOH. O exothermic O…
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Calculate the change in internal energy (ΔE) for a system that is giving off 3.0 kcal of heat and is changing from 1.00 L to 8.00 L in volume at a pressure of 2.00 atm. (Remember that 101.3 J = 1 L∙atm; 1 cal = 4.18 J)
A calorimeter contains 16.0 mLmL of water at 12.5 ∘C∘C . When 1.40 gg of XX (a substance with a molar mass of 75.0 g/molg/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq)X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C∘C . Calculate the enthalpy change, ΔHΔ�, for this reaction per mole of XX. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)J/(g⋅∘C)], that density of water is 1.00 g/mLg/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures.