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A piece of unknown substance weighs 57.2 g and requires 3210 ) to increase its temperature...
20. A piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from 23.2 °C to 89.6 °C. What is the specific heat of the substance?
Calculate the amount of heat in J required to increase the temperature of 25.0 grams of water from 25. °C to 50.0 °C. ice Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol Specific Heat (J/g (state) °C) helium He(s) 5.193 water H2O(1) 4.184 ethanol C2H60(1) 2.376 H2O(s) 2.093 (at -10 °C) water vapor H2O(g) 1.864 nitrogen N2(8) 1.040 air 1.007 oxygen O2(8) 0.918 aluminum Al(s) 0.897 carbon CO2(8) 0.853 dioxide argon Ar(s) 0.522 iron Fe(s)...
QUESTION 7 A 437.2 g sample of an unknown substance requires 8460to increase its temperature from 19.3 °C to 68.9 °C. The specific heat of the substance is __J/g °C. QUESTION 8 A 437.2 g sample of an unknown substance requires 8460 ) to increase its temperature from 19.3 °C to 68.9 °C. According to table 5.1 in the text, the sample may be copper lead aluminum iron QUESTION 9 A 30.0 g piece of aluminum (C = 0.897 J/g...
22:02 4 Exit Question 8 4 pts ice A piece of aluminum lost 100.0 J of heat upon cooling from 50.0°C to 25.0°C. Calculate the mass of aluminum in grams. Round your final answer to three (3) significant figures. Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol Specific Heat (J/g (state) °C) helium He(g) 5.193 water H2O(1) 4.184 ethanol C2H00) 2.376 H2O(s) 2.093 (at -10 °C) water vapor H2O(g) 1.864 nitrogen N2(8) 1.040 air 1.007...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
Please help! QUESTION 3 The specific heat (s) of a substance is the amount of heat (9) required to raise the temperature of one gram of the substance by one degree Celsius. Calculation of heat (q) absorbed or released: q=sxm x At where At = tfinal - tinitial TABLE 6.2 The Specific Heats of Some Common Substances Specific Heat Substance (J/g. "C) AI 0.900 Au 0.129 C (graphite) 0.720 C (diamond) 0.502 Cu 0.385 Fe Hg 0.139 HO 4.184 C,H,OH...
Review Constants Periodic Part A It takes 45.0J to raise the temperature of an 10.6 g piece of unknown metal from 13.0°C to 24.5°C. What is the specific heat for the metal? Express your answer with the appropriate units. View Available Hint(s) TEMA C.- Value Units Submit Parts B and The next two questions pertain to silver. They have nothing to do with unknown metal described in Part A - Part B How much energy would it take to raise...
(7 pts.) Calculate the heat absorbed when 4.20 g of H2 are produced according to the following equation. CH3OH (g) → CO(g) + 2 H2(g) AH = 90.2 kJ (7 pts.) When one adds 1.475 kJ of heat energy to a sample of gold, the temperature goes from 12.5 °C to 84.6 °C. Calculate the mass of the sample of gold. Gold has a specific heat capacity of 0.129 J/g.°C. (6 pts.) 10. Write the thermochemical equation for the standard...