When 12.0 g (0.100 mol) of MgSO,(s) is dissolved in water in a constant pressure calorimeter, the temperature increases from 20.0 to 38.2°C. The heat capacity of the calorimeter and all its contents is 500. JK-1. What is the enthalpy of dissolution of magnesium sulfate (in kJ mol-1)? А 107 B 91.0 -91.0 D -107

When 12.0 g (0.100 mol) of MgSO,(s) is dissolved in water in a constant pressure calorimeter, the temperature increases from 20.0 to 38.2°C. The heat capacity of the calorimeter and all its contents is 500. JK-1. What is the enthalpy of dissolution of magnesium sulfate (in kJ mol-1)? А 107 B 91.0 -91.0 D -107

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...

See similar textbooks

Similar questions

Mg(s) + 1/2 O2(g) -> MgO(s). Determind the value of the standard enthalphy change for the reaction. Mg(s) + 2 HCI(aq) -> MgCl2(aq) + H2(g). ∆Hrxn = -316 kJ mol-1 MgO(s) + 2 HCI(aq) -> MgCl2(aq) + H2O. ∆Hrxn = -45.7 kJ mol-1 H2(g) + 1/2 O2(g) -> H2O. ∆Hrxn = -286 kJ mol-1
hen the oxide of generic metal MM is heated at 25.0 ∘C25.0 ∘C, a negligible amount of MM is produced. MO2(s)↽−−⇀M(s)+O2(g)Δ?∘=290.6kJmolMO2(s)↽−−⇀M(s)+O2(g)ΔG∘=290.6kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s). chemical equation: MO2(s)+C(s)↽−−⇀M(s)+CO2(g) What is the thermodynamic equilbrium constant for the coupled reaction?
When ammonium chloride (NH_(4)Cl) is added to water, it breaks into positive and negative ions and decreases the temperature of the medium. Which statement is TRUE about this reaction?
For the reaction below, ΔrH° = −3307.9 kJ mol−1. What is the standard enthalpy of formation of FeS2(s)? 4 FeS2(s) + 11 O2(g) ⟶ 2 Fe2O3(s) + 8 SO2(g) Give your answer in kilojoules per mole (kJ mol−1). Data: Substance Standard enthalpyof formation (in kJ mol−1) Fe2O3(s) −833.1 SO2(g) −297.0 Please double check your answer.
B. Dissolution of Sodium Hydroxide mass of water: 200 g initial temperature of water: 20°C final temperature of water: 26.49°C qwater: 5430.832 J qdissolution: 5566.6028 J mass of solid NaOH: 5.0 g moles of solid NaOH: 0.125 mol ΔHof NaOH dissolution: -44.53 kJ/mol Is the dissolution of NaOH endothermic or exothermic? Justify your answer.
For each reaction equation, calculate the internal energy change, ΔE, of the reaction at 25 ∘C 2H2(g)+O2(g)⟶2H2O(l)Δ?=−571.6 kJ Δ?= kJ H2(g)+Cl2(g)⟶2HCl(g)Δ?=−184.6 kJ/mol Δ?= kJ
Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. Mg(OH), (s) + 2 HCI(g) → MgCl, (s) + 2 H,O(g) AHixn kJ
Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. C₂H₂ (g) + 50₂ (g) - AHixn = 3 CO₂(g) + 4 H₂O(g) kJ
In the following experiment, solid CaCl2 (M = 110.98 g/mol) is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔsolnH = ? kJ mol−1A 4.00 g sample of CaCl2 is added to a coffee-cup calorimeter containing 125 g of H2O. The initial temperature of water in the calorimeter is 22.0°C and the final temperature is 27.5°C. What is the enthalpy change for the dissolution reaction (ΔsolnH) in kJ per mole of CaCl2? Assume the specific heat capacity of the solution is the same as water (Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.
What is ΔHrxn if mixing 50.0 mL of 0.500 M HCl (aq) with 50.0 mL of 0.500 M NaOH (aq), both initially at 24.0 °C results in a Tmix of 27.3 °C? Assume that the reaction goes 100% HCl (aq) + NaOH (aq) → H2O (l) + NaCl(aq) **answer in kJ/mol of H2O produced
Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. H, O(g)+C(graphite)(s) → H, (g)+CO(g) kJ AHixn
Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ