Final answer:
The amount of heat needed can be calculated using the formula Q = mcΔT, where Q is the heat, m is the mass, c is the specific heat, and ΔT is the change in temperature. For a 35.0 g sample of iron heated from 25 °C to 35 °C, the amount of heat required is 157.15 J.
Step-by-step explanation:
To calculate the heat involved when a sample of iron is heated, we can use the formula Q = mcΔT, where Q is the heat, m is the mass, c is the specific heat, and ΔT is the change in temperature. In this case, the mass of the iron is 35.0 g, and the change in temperature is 10 °C (35 °C - 25 °C). The specific heat of iron (0.449 J/g.°C) can be used to calculate the heat. Plugging in the values: Q = (35.0 g)(0.449 J/g.°C)(10 °C) = 157.15 J.
To determine the heat required to raise the temperature of a 35.0 g iron sample from 25 °C to 35 °C, the formula q = mc∆T is used with the specific heat of iron (0.107 cal/g°C), resulting in 37.45 calories needed.
To calculate how many calories are needed to heat a 35.0 g sample of iron from 25 °C to 35 °C, we can use the formula q = mc∆T, where q is the heat energy in calories, m is the mass in grams, c is the specific heat capacity in cal/g°C, and ∆T is the change in temperature in degrees Celsius. The specific heat capacity of iron is approximately 0.449 J/g°C, which is equivalent to 0.107 cal/g°C (since 1 calorie = 4.184 joules).
First, calculate the change in temperature (∆T):
∆T = Tfinal - Tinitial = 35 °C - 25 °C = 10 °C
Using the given mass, the specific heat capacity for iron, and the change in temperature, the calculation is:
q = (35.0 g) × (0.107 cal/g°C) × (10 °C)
q = 37.45 calories
Therefore, 37.45 calories of heat are needed to raise the temperature of a 35.0 g sample of iron from 25 °C to 35 °C.