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**Need a little help, as I seem to have gotten confused.**

Looking over past exam questions for the heat capacity of a calorimeter, this one is the one I am looking at :

Looking over past exam questions for the heat capacity of a calorimeter, this one is the one I am looking at :

**A sample of the sugar fructose (C6H12O6) of mass 0.900 gwas placed in a calorimeter and**

ignited inthe presence of excess oxygen, at the saturation vapour pressure of water and at

constant volume.The temperature rose by 1.4 K.

The calorimeter had previously been calibrated by passing an electrical current through a heating

tape for 100 s. The power supplied to the tape was 500 W and the temperature of the calorimeter

rose by 5 K

ignited inthe presence of excess oxygen, at the saturation vapour pressure of water and at

constant volume.The temperature rose by 1.4 K.

The calorimeter had previously been calibrated by passing an electrical current through a heating

tape for 100 s. The power supplied to the tape was 500 W and the temperature of the calorimeter

rose by 5 K

**Right. The reason I am confused, is the textbook I've been reading from had similar worked examples, however they didn't have any values in watts. They have in Ampere and Volts.**

As far as I am aware 1 watt is equal to 1j/s..

As far as I am aware 1 watt is equal to 1j/s..

**So to work the heat capacity of the calorimeter,**

would i:

would i:

**1) 500W*60 to get to 8.3 J/s**

2) then multiply by 100s and divide by the 5K.

3) then multiply this answer by 1.4k, to get 233.3 joules.

4) Finally, divide by 1000, to get the heat capacity of the calorimeter at 0.23KJ?

2) then multiply by 100s and divide by the 5K.

3) then multiply this answer by 1.4k, to get 233.3 joules.

4) Finally, divide by 1000, to get the heat capacity of the calorimeter at 0.23KJ?

**Or am I way off?**