ThermochemistryHard

Question

Assume that for a domestic hot water supply, 160 kg of water per day must be heated from 10oC to 60oC and gaseous fuel propane, C3H8, is used for this purpose. What volume of propane gas at STP would have to be used for heating domestic water, with efficiency of 40%? Heat of combustion of propane is −500 kcal/mol and specific heat capacity of water is 1.0 cal/K-g.

Options

A.896 L
B.908 L
C.896 m3
D.908 m3

Solution

Heat liberated from propane = Heat absorbed by water

Or, $n \times 500 \times 10^{3} \times \frac{40}{100} = 160 \times 10^{3} \times 1 \times 50 \Rightarrow n = 40$

Create a free account to view solution

View Solution Free
Topic: Thermochemistry·Practice all Thermochemistry questions

More Thermochemistry Questions

Reactions involving gold have been of particular interest to a chemist. Consider the following reactions.Au(OH)3 + 4HCl ...ᐃHof of water is - 285.5 kJ mol-1. if enthalpy of neutralisation of monoacid strong base is - 57.3 kJ mol-1, &#512...The ᐃHof for CO2(g), CO(g) and H2O(g) are - 393.5 - 110.5 and 241.8 kJ mol -1 respectively. The standard enthaly c...The bond energy (in kcal mol-1) of a C - C single bond is approximately...For the given reactionsSiO2 + 4HF → SiF4 + 2H2O, ᐃH = -10.17 kcalSiO2 + 4HCl → SiCl4 + 2H2O, ᐃH ...