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Question

The standard heat of combustion of propane is $$-2220.1\ kJ/mol$$. The standard heat of vaporization of liquid water is $$44\ kJ/mol$$. What is the $$\triangle H^{o}$$ of the reaction :
$$C_{3} H_{8} (g)+ 5O_{2} (g) \rightarrow 3CO_{2} (g) + 4H_{2} O (g)$$?

A
$$-2396.1\ kJ$$
B
$$-2044.1\ kJ$$
C
$$-2220.1\ kJ$$
D
$$-2176.1\ kJ$$
Solution
Verified by Toppr

Correct option is B. $$-2044.1\ kJ$$

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Similar Questions
Q1
Propane and oxygen react according to the equation: C3H8(g)+5O2(g)3CO2(g)+4H2O(g)
If two moles of C3H8(g) is used in the above reaction then determine how many grams of water will produce after the complete combustion?
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Q2

C3H8(g)+5O2(g)3CO2(g)+4H2O(l)

The combustion of propane, C3H8(g), proceeds according to the equation above. In the complete combustion of 44.0 grams of propane, determine how many grams of water will be formed.
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Q3
Calculate the heat of combustion (kJ) of propane, C3H8 using the listed standard enthalpy of reaction data:
C3H8(g)+5O2(g)3CO2(g)+4H2O(g)
3C(s)+4H2(g)C3H8(g)ΔH/kJ=103.8
C(s)+O2(g)CO2(g)ΔH/kJ=393.5
H2(g)+1/2O2(g)H2O(g)ΔH/kJ=241.8
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Q4
Consider the following combustion reaction:
C3H8(g)+5O2(g)3CO2(g)+4H2O(g)
At STP (atm), when 64.4 L of propane is reacted with 87.0 L of oxygen gas, volume of the CO2 gas produced is:
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Q5
The heats of formaton of CO2(g) and H2O(I) are -394 kJ/mole and -285.8 kJ/mole respectively. Using the data for the following combustion reaction, calculate the heat of formation of C3H8(g).
C3H8(g)+5O2(g)3CO2(g)+4H2O(l) ; ΔHrxn=2221.6kJ

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