A piece of metal weighing 98.4 g with a specific heat of 0.46 Jg¹°C at 1028.6 °C is dunked into a beaker containing 475.9 1 ml of water at 25 C. Assuming all heat is absorbed by the water, what will be the final temperature of the water expressed on = 418479 0 Per = 1g/ml Select one: 0 a 47.3°C Ob 320 Oc 33°C Od 19°C of the following relationships, if plotted yields a straight Clear my choice

105 mL of H2 O is initially at room temperature (22.0° C). A chilled steel rod at 2.0° C is placed in the water. If the final temperature of the system is 21.3 °C, what is the mass of the steel bar? Specific heat of water = 4.18 J/g.°C Specific heat of steel = 0.452 J/g.°C

Find the heat of metal and the specific heat capacity (below are the values)   Mass of metal 23.2038g volume of water 100.0 mL Initial temperature of water 25.01 degrees Celcius Initial temperature of Metal 200.00 degrees celcius Max final temperature of water and metal 28.75 degrees celcius mass of water 99.71g change in temperature for water 3.74 degrees celcius Heat of water 156 Joules Change in temperature for metal -171.25 Degrees celcius

How much heat (in kJ) will be absorbed by a 75.9 g piece of aluminum (specific heat = 0.930 J/g･°C) as it changes temperature from 23.0°C to 67.0°C?

I got these wrong, and I'm unsure how to get to the correct answer, please help me!

A hot lump of 47.9 g of copper at an initial temperature of 99.7 °C is placed in 50.0 mL H₂O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g-°C)? Assume no heat is lost to surroundings. Tiinal = °℃

A piece of metal weighing 146.7 g was heated from 32.0 °C to 56.2 °C. If the amount of heat needed was 1363.3 J, calculate the specific heat of the metal. What is the identity of the metal? 20 Specific Heats of Selected Metals Smetal, J/g-°C Metal 0.901 Smetal, J/g-°C 0.449 Metal Al Fe Cu 0.384 Ni 0.444 Si 0.711 Sn 0.226 Zn 0.389 Mn 1.02

The specific heat of a certain type of metal is 0.128 J/(g.°C). What is the final temperature if 305 J of heat is added to 58.8 g of this metal, initially at 20.0 °C? Trinal 130.53 °C

The combustion of butane produces heat according to the equation2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(l)               ΔH  = -5,314.0 kJ   What is the change in heat if 13.98 g C4H10 (58.12g/mol) reacts?(Answer should have one place after the decimal. Watch the sign)

As a lab experiment, a 10.0 g sample of iron metal, specific heat = 0.444 J/ g*oC, is heated from 22oC to 1600oC and then added to 50 g of water at 22oC.  What is the final temperature of the water, assuming no heat is lost to the surroundings? Specific heat of water = 4.184 J/ g*oC.