6. The temperature of a sample of iron with a mass of 10.0 g changed from 50.4°C to 25.0°C with the release of 47 Joules of heat. What is the specific heat of iron? (p=a (m)(AT)

1. How much heat, in joules and in calories, must be added to a 75.3 g chromium block with a specific heat of 0.450 J/g·°C to increase its temperature from 25°C to its melting temperature of 1907°C?  J  =  cal = 2. A piece of unknown substance weighs 45.9 g and requires 2730 J to increase its temperature from 23.1°C to 88.9°C. (a) What is the specific heat (in J/g·°C) of the substance?  J/g·°C (b) If it is one of the substances found in the table below, what is its likely identity? Specific Heats of Common Substances at 25°C and 1 bar Substance Symbol (state) Specific Heat (J/g·°C) gold Au(s) 0.129 copper Cu(s) 0.384 iron Fe(s) 0.449 argon Ar(g) 0.521 silicon Si(s) 0.712 carbon dioxide CO2(g) 0.843 aluminum Al(s) 0.904 nitrogen N2(g) 1.039 water H2O(l) 4.1801 helium He(g) 5.196

A 95.5 g piece of copper (specific heat 0.380 J/g･°C) is heated and then placed into 400.0 g of water initially at 20.7°C. The water increases in temperature to 22.2°C. What is the initial temperature (in °C) of the copper? (The specific heat of water is 4.184 J/g･°C).

A metal is thought to be copper or gold. When 18 g of the metal absorbs 58 cal, its temperature rises by 35 ̊C. a) What is the specific heat, in cal/g ̊C, of the metal? b) Would you identify the metal as copper or gold?