Question
In: Chemistry
In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon...
In the presence of excess oxygen, methane gas burns in a
constant-pressure system to yield carbon dioxide and water:
CH4 (g) + 2O2 (g) → CO2 (g) +
2H2O (l) ΔH = -890.0 kJ
Calculate the value of q (kJ) in this exothermic reaction when 1.00
g of methane is combusted at constant pressure.
| a. -55.6 kJ |
| b. -5.56 × 104kJ |
| c. -0.0180 kJ |
| d. 55.6 kJ |
| e. 0.0180 kJ |
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...
Methane, CH4, burns completely in oxygen to yield carbon dioxide and water. 1. how many grams...
Methane, CH4, burns completely in oxygen to yield carbon dioxide
and water. 1. how many grams of carbon dioxide can be formed from
16.0g of methane and 48.0g of oxygen?
2. how much excess reagent will be left unreacted?
3. if only 30.0g of carbon dioxide are formed, what is the
percent yield of the reaction?
a mixture of oxygen, hydrogen, carbon dioxide and methane gases have a total pressure of 1.3...
a mixture of oxygen, hydrogen, carbon dioxide and
methane gases have a total pressure of 1.3 ATM. if the partial
pressure of hydrogen is 2.4 PSI, the partial pressure of carbon
dioxide is 110 torr can the partial pressure of methane is 0.22
ATM, how many mmhg does oxygen exert?
Using The Degree of Advancement Variable Methane and oxygen react in the presence of a catalyst...
Using The Degree of Advancement Variable
Methane and oxygen react in the presence of a catalyst to give
formaldehyde. In a parallel reaction, methane is oxidized to carbon
dioxide and water:
CH4 + O2 = HCHO + H2O
CH4 + O2 = CO2 + H2O
The reactor feed contains equimolar amounts of methane and
oxygen. Assume as a base a feed of 100 mol / s.
The methane conversion fraction is 0.90 and the
formaldehyde yield fraction is 0.855. Use...
Calculate the theoretical flame temperature for CO gas burned at constant pressure with 100% excess air,...
Calculate the theoretical flame temperature for CO gas burned
at constant pressure with 100% excess air, when the reactants enter
at 100°C.
Please show work, do not copy the
solution founded. show your solution! if you can not answer this
question, then do not attempt to copy others' work.
A 44.39 gram sample of iron is heated in the presence of excess oxygen. A metal...
A 44.39 gram sample of iron is heated in the presence of excess
oxygen. A metal oxide is formed with a mass of 63.46 g. Determine
the empirical formula of the metal oxide. Enter the elements in the
order Fe, O empirical formula =
If 2.00 g hydrogen gas is reacted with 28.0 g of oxygen gas in the presence...
If 2.00 g hydrogen gas is reacted with 28.0 g of oxygen gas in
the presence of 0.40 Pt catalyst and produces 5.00 g water. What is
the limiting reagent, theoretical yield of water in moles.and
percent yield? Please show all work.
Methane is completely burned with 30% excess air, with 20% of the carbon transforming to CO....
Methane is completely burned with 30% excess air, with 20% of
the carbon transforming to CO.
a) What is the molar composition of the stack gas on a dry
basis?
b) Estimate the partial pressure of the CO in the stack gas if the
barometer read 750 mmHg.
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