Question

A blacksmith heats a 1,540 g iron horseshoe to a temperature of 1445°C before dropping it into 4,280 g of water at 23.1°C. If the specific heat of iron is 0.4494 J / g °C, and the water absorbs 947,000 J of energy from the horseshoe, what is the final temperature of the horseshoe-water system after mixing?

Answer 1

We can use the equation Q1 + Q2 = 0 to solve for the final temperature of the horseshoe-water system after mixing.

Q1 is the amount of heat lost by the horseshoe, and Q2 is the amount of heat gained by the water. We can calculate Q1 using the formula:

Q1 = m1 * c1 * ΔT1

where m1 is the mass of the horseshoe (1540 g), c1 is the specific heat of iron (0.4494 J/g°C), and ΔT1 is the change in.

Answer 2

dang, dang Diggity. Dang dang dang dang Diggity. Dang dang the answers. Probably like at least one.