4.80g of Ch4 is mixed with 17.6g of co2 in a 9.00l
flask at temprature of...
4.80g of Ch4 is mixed with 17.6g of co2 in a 9.00l
flask at temprature of 67.2 degree celsius. what is the total
pressure of the flask.(Assume there is no reaction)
Question 2 options:
For the reaction CH4 + O2 →CO2 + H2OCH4 + O2 →CO2 +
H2O
what are the coefficients for each reactant or product?
a. CH4
b. O2
c. CO2
d. H2O
Question 3 (2 points)
Question 3 options:
For the reaction NaOH + AlCl3 →NaCl + Al(OH)3NaOH +
AlCl3 →NaCl + Al(OH)
what are the coefficients for each reactant or product?
a. NaOH
b. AlCl3
c. NaCl
d. Al(OH)3
Question 4 (2 points)
Question 4 options:
For the reaction H2O2...
An initial concentration of CO2 equal to 1.00 M is in
a flask at 25°. What is the equilibrium concentration of
CO2? The Kc is 3.2 ´ 10-3 at 25°C.
SnO2(s) + 2 CO(g) D Sn(s) + 2 CO2(g) Hrxn =
–36 kJ
Annual emissions of CO2, CH4 and
N2O in the USA are estimated to be 6,000
MtCO2/yr, 36 MtCH4/yr and 1.75
MtN2O/yr.
What are the impacts of these gases emitted from the USA over a
100-year time horizon?
Find the total equivalent CO2 emissions.
16.05 g of methane (CH4) gas is mixed with 101.12 g of oxygen
(O2) gas. The mixture is ignited. After a bright flash and a loud
bang, some water droplets form on the inside of the reaction
vessel.
A) Write the balanced chemical reaction for the combustion of
methane .
B) How many moles of water can you make?
C) How many moles of CO2 can you make?
D) Will anything be left over? What?
Yes, there will be oxygen...
4a. For the following reaction, 3.96 grams of
carbon tetrachloride are mixed with excess
methane (CH4) . The reaction yields
3.67 grams of dichloromethane
(CH2Cl2) .
methane (CH4) ( g ) +
carbon tetrachloride ( g )
-------> dichloromethane
(CH2Cl2) ( g )
What is the theoretical yield of dichloromethane
(CH2Cl2) ?
_______ grams
What is the percent yield for this reaction ?
________%
4b. For the following reaction, 5.03 grams of
silver nitrate are mixed with excess
copper(II) chloride....
Given the following chemical equations:
I. CH4 + 2O2
→ CO2 + 2H2O (1.25 L of
CH4 with density = 0.656 g/L)
II. 6CO2 + 6H2O
→ C6H12O6 (7.25 g of
CO2 )
Which equation will have the highest number of carbon atoms
produced based on the information given next to each chemical
equation?
A. I
B. II
Be sure to answer all parts. Determine the mole fractions and
partial pressures of CO2, CH4, and He in a sample of gas that
contains 1.25 moles of CO2, 1.49 moles of CH4, and 3.61 moles of
He, and in which the total pressure is 5.78 atm.
ΧCO2 =
PCO2 =-----atm
ΧCH4 =
PCH4 = -----atm
ΧHe =
PHe =---- atm
The volumetric analysis of a certain fuel is given as
C2H6 22.6%
CH4 73.6%
CO2 2.4%
N2 1.4%
For 100 moles and the combustion ofair is dry and in 25%
excess
Calculate
1) The molecular weight of the combustion products
2) The total gas volume for complete combustion at 260oC, 1
bar
3) The dry flue gas analysis based on CO2, O2 and N2.
If 01.2 KOH is mixed with 0.05g of CO2 according to the
following equation, 2KOH + CO2 -----> K2CO3+ H2O
a. What is the limiting reactant? ______________________
b. How many grams of K2CO3can be produced? ________________
c. What is the excess reactant? __________________
d. If 0.16g of K2CO3isolated, what is the % yield?
Two gases are mixed in a 10.0 L fixed volume flask: 2.0L of O2
at 2.00atm and 8.0L of N2 at 3.00 atm. A. Calculate the partial
pressure for each gas and the total pressure. B. How much (volume
in liters) argon at 5.0 atm must be added to the 10.0L flask to
lower the mole fraction of nitrogen to .5? C. What is the total
pressure of the mixture from Part B?