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The temperature of the substance increases by 16.7 °C when 1.0 x 10¹ cal of heat is added to the substance. What is the most likely identity of the substance? aluminum iron water silver lead copper Substance lead silver copper iron aluminum water Specific heat (cal/g °C) 0.031 0.058 0.092 0.107 0.216 1.000
Specific heat is a more precise measure. The term is used to refer to the amount of heat that when added to or removed from one gram of the substance, produces a change in its temperature of 1 degree Celsius. Water has the highest specific heat capacity of all liquids. It is one calorie, or 4.184 Joules.
This heat is called the Latent heat. is the equation where L is the Latent heat and is material specific. How much heat is required to take water (mass of .55 kg) from -20 to 20 C? L for ice to water is 33.5 * 104 J/kg. the specific heat of ice is 2090 J/(kg*C).and for water is 4186 J/(kg*C).
Conclusion: Sand heats up faster than water because it has a lower specific heat. Water has a specific heat, which requires one calorie of energy to raise the temperature of one gram of water by one degree Celsius. Sand has a lower specific heat. It takes .19 calories per gram to raise the temperature of the sand by 1 degree Celsius.
The specific heat of water is 4.184 J/g °C. S = (J/g °C) The specific heats of several metals are given in the table. Metal Specific heat (J/g · °C) palladium 0.239 lead 0.130 zinc 0.388 aluminum 0.897 nickel 0.444 Based on the calculated specific heat, what is the identity of the mystery metal? O lead zinc O nickel aluminum O palladium EOOO O
(The specific heat capacity of liquid water is 4.184 J/g ⋅ K. The enthalpy of fusion of ice at 0 °C is 333 J/g.) A 29.41 gram piece of metal (specific heat, 0.51 J/g•°C) with an initial temperature of 46.2°C is added to 289.35 grams of water (specific heat, 4.184 J/g•°C) initially at 36.4°C.
10.71 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
A cubic piece of platinum metal (specific heat capacity = 0.1256 J/°C･g) at 200.0°C is dropped into 1.00 L of deuterium oxide ('heavy water,' specific heat capacity = 4.211 J/°C･g) at 25.5°C. The final temperature of the platinum and deuterium oxide mixture is 42.9°C.
The specific heat of water is 1.0 cal/g • K, its heat of fusion is 80 cal/g, and its heat of vaporization is 539 cal/g. O 1.4 kcal O 1.2 kcal O 1.1 kcal O 1.3 kcal If 2.0 g of water at 0.00°C is to be vaporized, how much heat must be added to it?
The specific heat of water is 4.184 1/g- "C. aig - "C) The specific heats of several metals are given in the table. Metal Specific heat g- "C) palladium lead 0239 0.130 ine 0388 aluminum O.897 nickel 0.444 Based on the caloulated specific heat, what in the identity of the mystery metal lead iel wmium Oplladm 0000O