Question

Find the volume of methane measured at 298K and 1.19 atm required to convert 1.41L of...

Find the volume of methane measured at 298K and 1.19 atm required to convert 1.41L of water vapor at 373K.

The heat combustion of CH4 is 890.4 kJ/mole and the heat capacity of H2O is 75.2J/mol x K.

Homework Answers

Answer #1

let the moles of methane required =x

Heat this is supplied= 890.4*x

It is assumed that the water vapor has to be evaporated at 373K

hence latent heat of vaporization of water= 2277 j/g

Density of water vapor = 18/22.4 ( at STP) =18/22.4 g/L (at STP)

density of water vapor at 373K= 0.803571 g/L*273.15/373= 0.588 g/L

mass of 1.41 L of water= 1.41*0.588 =0.83 gm

Latetn heat of water= 2277 (j/g)*0.83=1890 joules

890.4*1000x= 1890 ( heatt of combustion= heat required to convert water into vapor)

x= 1890/(890.4*1000)=0.002123 moles

from PV= nRT    V=volume of methane= nRT/P = 0.002123*0.08206*298/1.19=0.043619 L

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Find the volume of methane measured at 298 K and 0.980 atm required to convert 0.920...
Find the volume of methane measured at 298 K and 0.980 atm required to convert 0.920 L of water at 298 K to water vapor at 373 K.
What volume of methane at STP would be required to convert a 2.0-kg block of ice...
What volume of methane at STP would be required to convert a 2.0-kg block of ice at −15 °C to water at 15 °C, assuming that no heat is lost? The heat of fusion for ice is 6.01 kJ mol−1. The heat capacity of ice is 2.108 J g−1 °C−1 and the heat of combustion for methane is 891 kJ mol−1.
A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has a pressure of 0.5015 atm...
A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has a pressure of 0.5015 atm when placed in a sealed container. The complete combustion of the mixture to carbon dioxide gas, CO2(g), and water vapor, H2O(g), was achieved by adding exactly enough oxygen gas, O2(g), to the container. The pressure of the product mixture in the sealed container is 2.421 atm. Calculate the mole fraction of methane in the initial mixture assuming the temperature and volume remain constant. Xch4=
A particular natural gas consists, in mole percents, of 83.0% CH4 (methane), 11.2% C2H6 (ethane), and...
A particular natural gas consists, in mole percents, of 83.0% CH4 (methane), 11.2% C2H6 (ethane), and 5.80% C3H8 (propane). A 385-L sample of this gas, measured at 25 ∘C and 729 mmHg , is burned in an excess of oxygen gas. How much heat, in kilojoules, is evolved in this combustion reaction? Express your answer with the appropriate units. The table shown here gives the enthalpy of combustion for three different hydrocarbon fuels to produce liquid water and gaseous carbon...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of methane is burned, 890.4 kj are give off to the surroundings. This means that the products have less energy stored in the bonds than the reactants. Thus, for the reaction: CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol. A) what is the enthalpy change when 2.00 mol of CH4 are burned? B)what is the enthalpy change when 22.4g...
the combustion of methane, CH4, in oxygen. CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l) the...
the combustion of methane, CH4, in oxygen. CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l) the heat of reaction at 77C and 1.00 atm is -885.5 kJ. what is the change in volume when 1.00 mol CH4 reacts with 2.00 mol O2. what is w for this change? calculate delta U (change in U) for the change indicated by the chemical equation
The gas methane, CH4(g), can be used in welding. When methane is burned in oxygen, the...
The gas methane, CH4(g), can be used in welding. When methane is burned in oxygen, the reaction is: CH4(g) + 2 O2(g)------>CO2(g) + 2 H2O(g)      (a) Using the following data, calculate ^H° for this reaction. ^H°f kJ mol-1:   CH4(g) = -74.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 ^H° = _____ kJ (b) Calculate the total heat capacity of 1 mol of CO2(g) and 2 mol of H2O(g), using CCO2(g) = 37.1 J K-1 mol-1 and CH2O(g) =...
A gaseous fuel mixture stored at 736 mm Hg and 298 K contains only methane (CH4)...
A gaseous fuel mixture stored at 736 mm Hg and 298 K contains only methane (CH4) and propane (C3H8). When 11.0 L of this fuel mixture is burned, it produces 722 kJ of heat. What is the mole fraction of methane in the mixture? (Assume that the water produced by the combustion is in the gaseous state.) ​
Methane gas is burned completely with 30% excess air in a furnace operating at one atmosphere....
Methane gas is burned completely with 30% excess air in a furnace operating at one atmosphere. Both the methane and air enter the furnace at 40ºC saturated with water vapor. The flue gas (furnace exhaust) leaves the furnace at 1000ºC. The flue gas then passes through a heat exchanger and emerges at 60ºC. If 260 mole/sec of methane fed to the furnace, how much heat is lost from the furnace, and how much heat is transferred in the heat exchanger?...
A fuel gas containing 40.00 mole% methane and the balance ethane is burned completely with pure...
A fuel gas containing 40.00 mole% methane and the balance ethane is burned completely with pure oxygen at 25.00°C, and the products are cooled to 25.00°C. A. Suppose the reactor is continuous. Take a basis of calculation of 1.000 mol/s of the fuel gas, assume some value for the percent excess oxygen fed to the reactor (the value you choose will not affect the results), and calculate -Q?(kW), the rate at which heat must be transferred from the reactor if...