Find initial temperature:
q: 19.73 kJ
m: 261 g
c: 0.385 j/gC
final temp: 33.0 C
Find initial temperature: q: 19.73 kJ m: 261 g c: 0.385 j/gC final temp: 33.0 C
The specific heat of copper is 0.385 J/gC . Calculate the final temperature when 25.0 g of copper metal at 100C is added to 50 mL of water at 20 C
It specific heat of copper is 0.385 J/(g.C). If 34.2 g of copper, initially at 24.0 C, absorbs 4.689 kJ, what will be the final temperature of the copper?
The specific heat of copper is 0.385 J/(g °C). If 34.2 g of copper, initially at 25°C, absorbs 7.880 kJ, what will be the final temperature of the copper? 25.4°C 598°C 27.8°C 623°C
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
Q=mcAT Creiger Quantity Heat = Mass x Specific Heat x (Temp final - Temp initial) A 30.0-8 sample of water at 7°C is mixed with a 50.0 g sample of water at 57°C. Calculate the immediate temperature just after mixing the two samples before any heat loss would occur? Temperature → _ _°C
Initial mass of ice = 150.89 g Final mass of ice = 99.69 g Initial temperature of water = 42 °C Final temperature of water = 0.4 °C Determine the mass of the ice that has melted. Determine the variation of the water temperature (ΔT). a) Calculate the energy (in J) released by 100 g of water when it cooled by ΔT. The specific heat capacity(c) of water is 4.18 J/(g°C). Use the formula Q = mcΔT and the mass...
If 400 J of heat were added to 100 g copper (specific heat = 0.385 J/g°C) and 400 J were added to 100 g of gold (specific heat = 0.129 J/g°C), which metal, copper or gold, would have the lower final temperature?
Copper metal has a specific heat of 0.385 J/g·°C. Calculate the amount of heat required to raise the temperature of 22.8 g of Cu from 20.0°C to 875°C. a. 1.0 × 10-2 J b. 1.97 × 10-5 J c. 7.51 kJ d. 329 J e. 10.5 kJ
a 5g piece of lead(specific heat .129 J/gC) is placed in 50ml of water(4.184). water temp incteases from 20 to 22 deg C lead final temp is also 22 deg C what was initial lead temp? please show work, equation used