Question
In: Chemistry
1.25 L of methane (CH_44) reacts with 1.65 L oxygen O_22(g) to produce 1.35 g of...
1.25 L of methane (CH_44) reacts with 1.65 L oxygen O_22(g) to produce 1.35 g of CO_22(g) (density of CH_44 = 0.656 g/L, density of O_22 = 1.43 g/L)
Using the following equation: CH_44(g) + 2O_22(g) → CO_22(g) + 2H_22O(l), determine the percent yield for the reaction.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Complete combustion of methane When methane (CH4CH4) burns, it reacts with oxygen gas to produce carbon...
Complete combustion of methane
When methane (CH4CH4) burns, it reacts with oxygen gas to
produce carbon dioxide and water. The unbalanced equation for this
reaction is
CH4(g)+O2(g)→CO2(g)+H2O(g)CH4(g)+O2(g)→CO2(g)+H2O(g)
This type of reaction is referred to as a complete
combustion reaction.
Part A
Part complete
What coefficients are needed to balance the equation for the
complete combustion of methane? Enter the coefficients in the order
CH4CH4, O2O2, CO2CO2, and H2OH2O, respectively.
Express your answer as four integers, separated by commas (e.g.,
1,2,3,4)....
When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The...
When methane (CH4) burns, it reacts with oxygen gas
to produce carbon dioxide and water.
The unbalanced equation for this
reaction is CH4(g)+O2(g) →
CO2(g)+H2O(g)
This type of reaction is referred
to as a complete combustion reaction.
B. What mass of carbon dioxide is produced from the
complete combustion of 5.00×10−3 (g) of methane? w/
units.
C. What mass of water is
produced from the complete combustion of
5.00×10−3 g of
methane? w/ units.
D. What mass of
oxygen is...
When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The...
When methane (CH4) burns, it reacts with oxygen gas to produce
carbon dioxide and water. The unbalanced equation for this reaction
is
CH4(g)+O2(g)→CO2(g)+H2O(g)
This type of reaction is referred to as a complete
combustion reaction.
Part B-What mass of carbon dioxide is produced from the complete
combustion of 3.00×10−3 g of methane?
Part C-What mass of water is produced from the complete
combustion of 3.00×10−3 g of methane?
Part D- What mass of oxygen is needed for the complete
combustion...
Propane gas, C3H8, reacts with oxygen to produce water and carbon dioxide. C3H8(g)+5O2(g)→3CO2(g)+4H2O(l) Part A How...
Propane gas, C3H8, reacts with oxygen to produce water and
carbon dioxide.
C3H8(g)+5O2(g)→3CO2(g)+4H2O(l)
Part A
How many moles of CO2 form when 3.70 mol of C3H8 completely
reacts?
Part B
How many grams of CO2 are produced from 17.4 g of propane
gas?
Part C
How many grams of CO2 can be produced when 43.4 g of C3H8
reacts?
Sulfur dioxide reacts with oxygen to produce sulfur trioxide. 150 g of sulfur dioxide is reacted...
Sulfur dioxide reacts with oxygen to produce sulfur trioxide.
150 g of sulfur dioxide is reacted with 50 g of oxygen. The
reaction proceeds until one reactant is completely consumed.
Write a balanced chemical equation or this
reaction.
What is the theoretical yield of sulfur trioxide?
What is the percent yield of sulfur trioxide if 180 g is actually
produced?
When 11.1 g of lead reacts with 3.81 L of oxygen gas, measured at 1.00 atm...
When 11.1 g of lead reacts with 3.81 L of oxygen gas, measured
at 1.00 atm and 25.0 °C, 11.8 kJ of heat is released at constant
pressure. What is ?H° for this reaction? (R = 0.0821 L • atm/(K •
mol))2 Pb (s) + O2 (g) ? 2 PbO (s)
When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture...
When the supply of oxygen is limited, iron metal reacts with
oxygen to produce a mixture of FeO and Fe2O3 . In a certain
experiment, 20.00 g iron metal was reacted with 11.31 g oxygen gas.
After the experiment, the iron was totally consumed, and 3.91 g
oxygen gas remained. Calculate the amounts of FeO and Fe2O3 formed
in this experiment.
Nitrogen gas reacts with oxygen gas to form dinitrogen tetroxide. N2 (g) + 2 O2 (g)...
Nitrogen gas reacts with oxygen gas to form dinitrogen
tetroxide.
N2 (g) + 2 O2 (g) → N2O4 (g)
A 1.8 L reaction vessel, initially at 298 K, contains nitrogen
gas at a partial pressure of 337 mmHg and oxygen gas at a partial
pressure of 445 mmHg .
What is the pressure of N2O4 in the reaction vessel after the
reaction?
Enter your answer numerically, in terms of
mmHg.
Please show all work
A sample of 10.00 g of sodium reacts with oxygen to form 15.02 g of sodium...
A sample of 10.00 g of sodium reacts with oxygen to form 15.02 g
of sodium oxide (Na2O) and sodium peroxide
(Na2O2). Calculate the percent composition of
the mixture.
___% Na2O
___% Na2O2
16.05 g of methane (CH4) gas is mixed with 101.12 g of oxygen (O2) gas. The...
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...
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