What is the change in enthalpy in joules when 5.44 x 10- mol of AgCı dissolves in water according to the following chemical equation: AgCI(s) → Ag*(aq) + Cl¯(aq) AH = 65.5 kJ STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 6.022 x 102 5.44 x 104 65.5 0.0356 0.001 1000 35.6 3.56 x 106 0.00831 g Ag* J kJ g AgCI mol AgCI mol Ag* mol CI

What is the change in enthalpy in joules when 5.44 x 10- mol of AgCı dissolves in water according to the following chemical equation: AgCI(s) → Ag(aq) + Cl¯(aq) AH = 65.5 kJ STARTING AMOUNT ADD FACTOR ANSWER RESET ( ) 6.022 x 102 5.44 x 104 65.5 0.0356 0.001 1000 35.6 3.56 x 106 0.00831 g Ag* J kJ g AgCI mol AgCI mol Ag* mol CI

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

See similar textbooks

Similar questions

In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
The standard nthalpy of neutralization of a weak hydrogen cyanide acid, HCN (aq), by a stong base, NaOH (aq), is -12.1 kj/mol. Using Hess's Law and your experimental data on standard enthalpy of neutralization from Part A to calculate standard enthalpy of ionization of HCN (aq): HCN (aq) --> H+ (aq) + CN- (aq)), Hioniz (HCN) Part A= enthaply of neut= -60.066 kj/mol
Given that the standard enthalpy of formation of HI(aq) is −55 kJ mol−1, what is the value of ΔfH⦵(I−, aq)?
Given that the standard enthalpy of formation of HCl(aq) is −167 kJ mol−1, what is the value of ΔfH⦵(Cl−, aq)?
Given the following standard enthalpies of hydration; Mg 2 + (g) + (ag) Mg2+(aq); A110 - 1920KJ C-n (g) + (aq) CT (a q) ; All 0 - 364 KJ- and using the value of AHO for the reaction a!ready given; calculate the standard enthalpy of solution of magnesium chloride.
To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Write the balanced equation for the reaction between HCl and MgO.2. Which is the limiting reactant? Show your solution.3. Calculate heat released by the reaction, qrxn, in the calibration step (in kJ).
A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = J
What is the change in enthalpy in joules when 10.5g of AgCl (143.3g/mol) dissolves in water according to the following chemical equation: AgCl(s) à Ag+(aq) + Cl-(aq) ΔH°rxn = 65.5 kJ/mol
just to verify the answer rto 1 is increasing and 2 is increasing>??