let 1 denote Fe and 2 denote water
s1 = 0.452 J/g.oC
s2 = 4.186 J/g.oC
use,
m1*s1*(T-T1) = m2*s2*(T2-T)
32.0*0.452*(59.6 - 21.8) = m2*4.186*(63.5 - 59.6)
32.0*0.452*37.8= m2*4.186*3.9
546.7 = m2*16.32
m2 = 33.5 g
Answer : 33.5 g
Constants Periodic Table Part A A 32.0 g iron rod, initially at 21.8 °C, is submerged...
A 32.4 g iron rod, initially at 23.0°C, is submerged into an unknown mass of water at 63.4 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.1 °C. Part A What is the mass of the water? You may want to reference (Pages 259-264) Section 6.4 while completing this problem. Express your answer to two significant figures and include the appropriate units. m= Value Units Submit Request Answer
A 31.4 g iron rod, initially at 22.3 ∘C, is submerged into an unknown mass of water at 63.6 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 60.0 ∘C. What is the mass of the water?
A 32.1 g iron rod, initially at 22.8 ∘C, is submerged into an unknown mass of water at 64.0 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 58.8 ∘C. What is the mass of the water? Express your answer to two significant figures and include the appropriate units.
A 32.8 g iron rod, initially at 23.0 ∘C, is submerged into an unknown mass of water at 64.0 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.0 ∘C. What is the mass of the water?
A silver block, initially at 56.4 ∘C, is submerged into 100.0 g of water at 24.6 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.4 ∘C. What is the mass of the silver block?
A silver block, initially at 58.6 ∘C, is submerged into 100.0 g of water at 25.1 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.3 ∘C. What is the mass of the silver block? I got 122.53g is it wrong?
A silver block, initially at 58.2 ?C, is submerged into 100.0 g of water at 25.0 ?C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.6 ?C. -What is the mass of the silver block?
A) A silver block, initially at 55.4 ∘C, is submerged into 100.0 g of water at 25.3 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.8 ∘C. What is the mass of the silver block? B) Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.50×102kJ of heat? The balanced chemical equation is as follows: C(s)+O2(g)→CO2(g),ΔH∘rxn=−393.5kJ
A2.13 g lead weight, initially at 11.1°C, is submerged in 7.45 g of water at 52.5 °C in an insulated container Part A You may want to reference (Pages 373 - 379) Section 9.4 while completing this problem. What is the final temperature of both the weight and the water at thermal equilibrium? Express the temperature in Celsius to three significant figures. AEC RO? Submit Request Answer
A 31.6 g wafer of pure gold initially at 69.7 ∘C is submerged into 63.5 g of water at 27.1 ∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium? Express your answer using three significant figures.