Question

In a study of healthy young men, doing 20 push-ups in 1 minute burned an amount of energy per kg that for a 70.0-kg man corresponds to 8.06 calories (kcal). How much would a 70.0-kg man’s temperature rise if he did not lose any heat during that time?

(a) 0.23°C
(b) 0.35°C
(c) 0.50°C
(d) 0.62°C

Answer 1

The temperature rise would be 0.344 °C if no heat was lost during the push-ups.

Step-by-step explanation:

In order to calculate the rise in temperature, we can use the formula:

Q = mcΔT

Where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

Given that the amount of energy burned in 1 minute by doing 20 push-ups corresponds to 8.06 calories (kcal), we can convert this to joules (J) and use it as the value for Q.

Using the specific heat capacity of water (4.18 J/g·°C) and the mass of the person (70.0 kg), we can rearrange the formula to solve for ΔT:

ΔT = Q / (mc)

Plugging in the values, we get:

ΔT = (8.06 x 10^3 J) / (70.0 kg x 4.18 J/g·°C)

Simplifying the equation gives us: ΔT = 0.344 °C

So, the temperature would rise by 0.344 °C if no heat was lost during the push-ups.