Stoichiometry
How many grams of CO are needed to react with an excess of Fe2O3 to produce 558g Fe? The equation for the reaction is:
Fe2O3(s) + 3CO(g) → 3CO2(g) + 2Fe(s)
420.g CO
A calorimeter contained 75.0g of water at 16.95EC. A 93.3g sample of iron at 65.58°C was placed in it, giving a final temperature of 19.68°C for the system. Calculate the specific heat of the Fe.
.200 J/g °C
What is the acid and what is the base?
HNO3 + NaOH → H2O + NaNO3
Acid: HNO3, H2O
Base: NaOH, NaNO3
The temperature of a fixed mass of gas in a rigid container is increased from 28.00°C to 88.00°C. The initial pressure was 0.947 atm. What is the new pressure, after heating
P2 = 1.14atm
What is the equilibrium constant expression for the reaction?
3Fe(s) + 4 H2O(g) ⇌ Fe3O4 + H2(g)
[H2]-4/[H2O]-4
How many grams of butane (C4H10) must be burned in an excess of O2 to produce 15.0g of CO2 ?
2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
4.95g C4H10
The specific heat of elemental silicon is 0.702 J/gK. How many joules of heat are necessary to raise the temperature of 156g of silicon from 25.0°C to 37.5°C?
1368.9 J
name the Acid/Base
HC2H3O2
acetic acid
A gas is heated from 35.0°C to 100.5°C at a constant pressure of 1.00 atm. If the initial volume is 44.55mL. What will be the new volume.
V2= 54.0mL
Write the equilibrium expression for the following reaction
N2 (g) + 3 H2 (g) ↔ 2 NH2 (g)
K = [NH3]2/[N2][H2]3
How many grams of FeCr2O are required to produce 44.0 g of CO2 ?
4 FeCr2 O + 8 K2 CO3 + O2 --->2 Fe2 O3 + 8 K2 CrO4 + 8 CO2
135.9 g
A coffee-cup calorimeter is used to determine the specific heat of a metallic sample. The calorimeter is filled with 50.0mL of water at 25.0°C. A 36.5g sample of the metallic material is taken from water boiling at 100.0°C and placed in the calorimeter. The equilibrium temperature of the water and sample is 32.5°C. Calculate the specific heat of the metallic sample.
.637 J/g°C
name the Acid/Base
Strontium Hydroxide
Sr(OH-)2
The reaction will inflate the airbag to a volume of 15.0L, to a pressure of 0.950 atm, and a temperature of 37°C. what mass of Nitrogen gas will be in the bag.
15.7g
Write the equilibrium expression for the following reaction
I2 (s) + Cl2 (g) ↔ 2 ICl (g)
K= [ICI]2/[CI2]
Determine moles of Na S that can be prepared by the reaction of 0.2240 moles of sodium with 0.1320 moles of sulfur. Which reactant is the limiting reactant?
82 16 Na + S8 →8 Na2 S
.112 mol
If 3.358kJ of heat is added to a sample of water, the water’s temperature rises from 22.34°C to 36.74°C. A) Is this process endothermic or exothermic? B) How many grams of water were in the sample?
A. Endothermic
B.55.7g
Name four common bases
Detergents, Soap, Lye, Household ammonia
A gas is heated from -20.0°C to 57.0°C and the volume is increased from 2.00L to 4.50L. if the initial pressure is 0.125 atm, what is the final pressure (assume number of moles remains constant)
0.0725 atm
Write the equilibrium expression for the following reactions
NO2 (g) ↔ NO (g) + ½ O2 (g)
K= [NO] [O2] 1/2 /NO2
An element of x forms both a dichloride (XCl2) and a tetrachloride (XCI4). Treatment of 10.00g of XCI2 with excess chlorine forms 12.55g XCl4. Calculate the atomic mass of x and Identify x.
x=207.14 g/mol
When a mass of 182g of gold at some temperature is added to 22.1g of water at a temperature of 25.0ºC, the final temperature of the resulting mixture is 27.5ºC. If the specific heat of gold is 0.129 J/g∙ºC, what was the initial temperature of the gold sample?
37.35°C
Name 5 common Acids
Citric Acids, Absorbic acids, Vinegar, Carbonic acids, Lactic acids
A chemist is preparing to carry out a reaction at high pressure that requires 36.0 grams of hydrogen gas. The chemist pumps the hydrogen into a 12.4L rigid steel container at 25.0°C. To what pressure, in atm, must the hydrogen be compressed.
P = 35.2 atm
What equation gives the equilibrium constant for the following reaction?
N2(g)+O2(g)⇌2NO(g)
K= [PNO]2/PN2PO2