Home
Class 11
CHEMISTRY
When 1.3 g of butane C(4)H(10) was burnt...

When 1.3 g of butane `C_(4)H_(10)` was burnt in oxygen in a flame calorimeter containing 1.8 kg of water the temperature reose from 25.3 to `33.3^(@)C`. Calculate the enthalpy change for the combustion of 1 mol of butane?

Text Solution

AI Generated Solution

Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Higher Order Thinking Questions|16 Videos

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Competition File MCQ|158 Videos

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Revision Exercise (Long Answer Questions)|11 Videos

  • STRUCTURE OF ATOM

    MODERN PUBLICATION|Exercise Unit Practice Test|13 Videos

Similar Questions

Explore conceptually related problems

When 10 g of coal is burnt, it raises the temperature of 2 litres of water from 20^(@)C to 55^(@)C . Calculate the heat of combustion of fuel.

When 1.0 gm of fructose C_(6) H_(12) O_(6) (s) is burnt in oxygen in a bomb calorimeter, the temperature of the calorimeter water increases by 1.56^(@)C . If the heat capacity of the calorimeter and its contents is 10.0 kJ//^(@)C . Calculate the enthalpy of combustion of fructose at 298 K.

When 1.0g of oxalic acid (H_(2)C_(2)O_(4)) is burnt in a bomb calorimeter whose heat capacity is 8.75 kJ//K , the temperature increases by 0.312 K. The enthalpy of combustion of oxalic acid at 27^(@)C is

The combustion of 10g coke raised to temperature of 1.0kg water from 10^(@)C to 50^(@)C . Calculate the fuel value of cock. (Sp. heat of H_(2)O=1 cal//g) .

A quantity of 1.534 g of naphthanlene (C_(10) H_(g)) is burned in constant-volume bomb calorimeter. Consequently, the temperature of the water rises form 20.00^(@)C to 25.00^(@)C . If the quanity of water surrounding the calorimeter is exactly 3000g calculate the heat capcity of combustion of one mole of naphthalene (molar heat of combustion) Strategy : First calculate the heat changes for the water and the bomb calroimeter. using Finally, divide the value by the number of moles of naphthlene to calculate the molar heat of combusiton. Remember ot change 2.75 kJ^(@)C^(-1) to 2.75 xx 1000 j^(@)C C^(-1)

The combustion of 1.22 g benzoic acid (M=122) in a bomb calorimeter at 300 K caused a temperature rise of 3 K, While combustion of 0.88 g ethyl ethanote (M=88) caused a temperature rise of 2 K. Calculate the enthalapy change of combustion of CH_(3)COOC_(2)H_(5)(l) at 300 K. Given : Internal energy change of combustion for benzoic acid =-300kJ mol^(-1) at 300 K and R=8.3 JK^(-1)mol^(-1)

1 mole of naphthalene (C_(10)H_(8)) was burnt in oxygen gas at 25^(@)C at constant volume. The heat evolved was found to be 5138.8kJ. Calculate the heat of reaction at constant pressure. (R=8.3JK^(-1)" "mol^(-1))