Transcript What is the gram atomic mass of lead, Pb?

1) vocab word--the quantity of
heat needed to raise the
temperature of 1 g of water 1°C
2) vocab word--the amount of
energy required to raise the
temperature of 1 g of a
substance 1°C
1) calorie
2) specific heat capacity
1) vocab word--the amount of
energy required to raise the
temperature of 1 mol of a
substance 1°C
2) vocab word--the study of heat
changes that accompany
chemical reactions
1) molar heat capacity
2) thermochemistry
1) vocab word--a food calorie
2) vocab word--the SI unit of
heat
3) vocab word--chemical
reactions that include a heat
term
1) Calorie
2) Joule
3) thermochemical equation
1) vocab word--a device used to
measure the amount of heat
absorbed or released during
chemical or physical process
2) vocab word--the accurate
and precise measurement of
heat change for chemical and
physical processes
1) calorimeter
2) calorimetry
1) vocab word--measurement of
heat when using constantpressure calorimetry
2) vocab word--form of energy
that always flows from a warmer
object to a cooler object
1) enthalpy
2) heat
1) vocab word—process that
absorbs or gains heat from the
surroundings
2) vocab word—the ability or
capacity to do work
1) endothermic
2) energy
1) vocab word– the heat change
caused by the dissolution of one
mole of a substance
2) vocab word—the change in
enthalpy that accompanies the
formation of 1 mole of a
compound from its elements
1) Molar heat of solution
2) Standard heat of formation
1) vocab word—the heat
absorbed by 1 mole of a
substance in melting from a
solid to a liquid
2) vocab word—the amount of
heat necessary to vaporize 1
mole of a given liquid
1) Molar heat of fusion
2) Molar heat of vaporization
1) vocab word—process that
releases or loses heat to the
surroundings
2) vocab word—states that if you
add two or more thermochemical
equations to give a final equation,
then you can add the heats of
reaction to give the final heat of
reaction
1) exothermic
2) Hess’s Law
Endothermic or Exothermic?
exothermic
Endothermic or Exothermic?
endothermic
Endothermic or Exothermic?
exothermic
Endothermic or Exothermic?
endothermic
Endothermic or Exothermic?
endothermic
Endothermic or Exothermic?
exothermic
Endothermic or Exothermic?
exothermic
Endothermic or Exothermic?
endothermic
Endothermic or Exothermic
endothermic
Endothermic or Exothermic?
exothermic
Endothermic or Exothermic?
4 NO(g) + 6 H2O(l) → 4 NH3(g) + 5 O2(g)
ΔH = +1170 kJ
endothermic
NH3(g) + HCl(g) → NH4Cl(s)
ΔH = −176 kJ
exothermic
Endothermic or Exothermic?
H2(g) + ½ O2(g) → H2O(g) + 286 kJ
exothermic
HgO (s) + 90.7 kJ → Hg (l) + ½ O2 (g)
endothermic
A certain mass of water was
heated with 41,840 Joules, raising
its temperature from 22.0 °C
to 28.5 °C. Find the mass of water.
The specific heat of water is 4.184
J/(g·C°).
𝑞 = 𝑚 × ∆𝑇 × 𝐶
41840 J = m x 6.5C x 4.184 J/g C
m = 1538 g
If it takes 41.72 joules to heat a
piece of gold weighing 18.69 g from
10.0 °C to 27.0 °C, what is
the specific heat of the gold?
𝑞 = 𝑚 × ∆𝑇 × 𝐶
41.72 J = 18.69 g x 17C x C
C = 0.131 J/(g·C°)
Given that the specific heat
capacity of gold is 0.131
J/(g·C°), find its molar heat
capacity.
.131 𝐽 196.97𝑔 25.86 𝐽
×
=
𝑔∙℃
1 𝑚𝑜𝑙
𝑚𝑜𝑙 ∙ ℃
The temperature of 110 mL of water
rises from 25.0°C to 26.2°C when
0.10 mol of H+ is reacted with 0.10
mol of OH-. Calculate the amount
of heat released. Assume that the
denisty of the solution is 1.00
g/mL. The specific heat of water
is 4.184 J/(g·C°).
𝑞 = 𝑚 × ∆𝑇 × 𝐶
𝑞 = 110 𝑔 × 1.2℃ × 4.184 𝐽/𝑔 ∙ ℃; q = 552 J
How much heat energy is obtained
when 1 kg of ethane gas, C2H6, is
burned in oxygen according to the
equation:
2C2H6(g) + 7O2(g) → 4CO2(g) +
6H2O(l); ΔH = –3120 kJ
1 𝐾𝑔 ×
1000 𝑔
1 𝐾𝑔
×
1 𝑚𝑜𝑙
30.08 𝑔
×
−3120 𝑘𝐽
2 𝑚𝑜𝑙
= −51,862 𝑘𝐽
Determine the energy required
to boil 43.89 grams of water
at 100.0 °C. The ∆Hvapor of
H2O is 40.67 kJ/mol.
43.89 𝑔 ×
1 𝑚𝑜𝑙
18.02 𝑔
×
40.67 𝑘𝐽
1 𝑚𝑜𝑙
= 99.06 𝑘𝐽
What is the value for ΔH for the
following reaction?
CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g)
Given:
C(s) + O2(g) → CO2(g); ΔH = -393.5 kJ
S(s) + O2(g) → SO2(g); ΔH = -296.8 kJ
C(s) + 2 S(s) → CS2(l); ΔH = 87.9 kJ
Hess’s Law, double 2nd rxn, reverse 3rd rxn
H = -1075 kJ
CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
∆H° = –889.1 kJ
∆Hf° H2O(l) = –285.8 kJ/mol
∆Hf° CO2(g) = –393.3 kJ/mol
What is the standard heat of formation
of methane, ∆Hf° of CH4(g), as
calculated from the data above?
−889.1 = [−393.3 + 2(−285.8)] −[x + 2(0)]
x = ∆Hf° of CH4(g) = −75.8 kJ/mol