Question

How much heat is liberated at constant pressure when 1.41 g of potassium metal reacts with 6.52 mL of liquid iodine monochloride (d = 3.24 g/mL)? 2K(s) + ICl(l) → KCl(s) + KI(s) ΔH° = -740.71 kJ/mol a. 7.41 × 10^2 kJ b. 2.22 × 10^3 kJ c. 1.34 × 10^1 kJ d. 1.23 × 10^2 kJ e. 9.64 × 10^1 kJ

Name: how much heat is liberated at constant pressure when 141 g of potassium metal reacts with 652 ml of liquid iodine monochloride d 324 gml 2ks icll kcls kis h 74071 kjmol a 741 102 kj b 222 10 10723
Uploaded: 2022-06-02T14:06:48-08:00
Duration: 2 min 35 s
Channel: Shaiju T
Description: how much heat is liberated at constant pressure when 141 g of potassium metal reacts with 652 ml of liquid iodine monochloride d 324 gml 2ks icll kcls kis h 74071 kjmol a 741 102 kj b 222 10 10723

          How much heat is liberated at constant pressure when 1.41 g of potassium metal reacts with 6.52 mL of liquid iodine monochloride (d = 3.24 g/mL)?

2K(s) + ICl(l) → KCl(s) + KI(s)

ΔH° = -740.71 kJ/mol

a. 7.41 × 10^2 kJ
b. 2.22 × 10^3 kJ
c. 1.34 × 10^1 kJ
d. 1.23 × 10^2 kJ
e. 9.64 × 10^1 kJ

Added by Sofia P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Shaiju T

06/02/2022

Step 1

Given that the density of ICl is 3.24 g/mL and 6.52 mL of ICl is used: Mass of ICl = 6.52 mL * 3.24 g/mL = 21.12 g Moles of ICl = 21.12 g / 162.36 g/mol = 0.1301 mol Show more…

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How much heat is liberated at constant pressure when 1.41 g of potassium metal reacts with 6.52 mL of liquid iodine monochloride (d = 3.24 g/mL)? 2K(s) + ICl(l) → KCl(s) + KI(s) ΔH° = -740.71 kJ/mol a. 7.41 × 10^2 kJ b. 2.22 × 10^3 kJ c. 1.34 × 10^1 kJ d. 1.23 × 10^2 kJ e. 9.64 × 10^1 kJ