Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20∘C to 25∘C?
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- Reactions between acids and bases (neutralization reactions) are exothermic. You have a solution of an acid and a solution of a base, both at 23oC. If you mix the two solutions together, would you expect the final temperature to be greater or less than 23oC?arrow_forwardIn a constant‑pressure calorimeter, 65.0 mL65.0 mL of 0.330 M Ba(OH)20.330 M Ba(OH)2 was added to 65.0 mL65.0 mL of 0.660 M HCl.0.660 M HCl. The reaction caused the temperature of the solution to rise from 22.07 ∘C22.07 ∘C to 26.57 ∘C.26.57 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184J/g⋅°C,)4.184J/g⋅°C,) respectively), what is Δ?ΔH for this reaction (per mole H2OH2O produced)? Assume that the total volume is the sum of the individual volumes.arrow_forwardZinc metal reacts with HCl according to the following balanced equation: Zn(s) + 2HCI(aq) --> ZnCl2(aq) + H2(g) When 0.140 grams of Zn(s) is combined with an excess amount of HCI to make 50.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.60°C to 24.60°C. Find AH for this reaction in kJ/mol. Assume the density of the solution is 1.00 g/mL and the specific heat capacity of the solution is 4.184 J/g°C. Use an atomic weight of 65.38 g/mol for Zn Hints: -q(reaction) = q(solution) %3D AH = q/mol of limiting reagent %3D Do not type units with your answer. Type your answer to three significant figures. the proper If this question is on an exam on your scrap paper report your answer number of significant figures but still type three significant figures online. Your Answer:arrow_forward
- When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at standard-state conditions. What is the standard enthalpy of formation (ΔH°f) of HgO(s)?arrow_forwardCalcium carbonate can be decomposed upon applying heat with the following equation CaCO3(s) → CaO(s) + CO2(g) ΔH = +179.5kJ How much heat will be needed to decompose 30 g of calcium carbonate? AND What size container will be required (in L) to contain the carbon dioxide generated at 25ºC and 1.2 atm?arrow_forward(b) Calculate the enthalpy change for the reaction C(graphite) + 2 H2(g) → CH4(g) with the help of the enthalpy changes of the following reactions: C(graphite) + O2(g) → CO2(g) ∆H= -393.5 kJmol−1 H2(g) +1/2O2(g) → H2O(l) ∆H = -285.8 kJmol−1 CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.4 kJmol−1 The temperature is 25 ◦C in all instances.arrow_forward
- When 57.5 mL of 5.00 AgNO3 is added to a coffee-cup calorimeter containing 57.5 mL of 5.00 L AgI forms? Be sure your answer has the correct number of significant figures. g Agl x10 × NaI, with both solutions at 25 °C, what mass of Larrow_forwardCalculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. C;H¿(g) + 50,(g) → 3 CO,(g) + 4 H,O(g) ΔΗ kJ rxnarrow_forwardIn Part B of the experiment, a student mixes 30.0 mL of 1.1 M HC1(aq) with 30.0 mL of 1.000 M NaOH(aq) in a well-insultated calorimeter and observes that the temperature of the solution increases by 5.75 °C. These are similar conditions as the previous two problems. How many moles of water are formed? number of moles of water = molarrow_forward
- Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 48.1 g of KNO3KNO3 is dissolved in 229 g of water at 23.00 °C. KNO3(s)−→−−H2OK+(aq)+NO−3(aq) The temperature of the resulting solution decreases to 17.80 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? ?soln= kJ What is the enthalpy of the reaction? Δ?rxn= kJ/molarrow_forwardZinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s) + 2HCl(aq)-> ZnCl2(aq) + H2(g) When 0.115g of Zn(s) is combined with enough HCI to make 52.6mL of solution in a coffee - cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 21.5 °C to 24.7 °C. Part A Find \Delta Hrxn for this reaction as written. (Use 1.00 g/mL for the density of the solution and 4.18 J/(g°C) as the specific heat capacity.)arrow_forwardConstants Periodic Table Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HCI(aq)→ZnCl2 (aq) + H2 (g) When 0.112 g of Zn(s) is combined with enough HCl to make 51.5 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22,1°C to 24.1 C Part A Find A H,xn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4. 18 J/g. C as the specific heat capacity.) 國 AHxn = kJ/mol Submit Request Answer Provide Feedback Next> P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use Privacy Pollcy Permissions | Contact Us Vi 1:23arrow_forward
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