How many grams of silver are needed to absorb 1.00 kJ of energy changing the temperature 33.0 C to 41.8°C?

Answer 1

473.5 grams

#q = mcDeltaT#

q = heat energy (joules) m = mass (grams) c = specific heat (#"Joules"/"gram * Celsius"#) #DeltaT# = change in temperature

In this case: q = 1 KJ = 1000 J m = ? c = 0.24 #DeltaT# = 41.8 - 33 = 8.8

#q = mcDeltaT# 1000 = (m)(0.24)(8.8) 1000 = (m)(2.112) m = 473.5

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Answer 2

Wyatt Atkins

To calculate the heat absorbed by silver, use the formula: q = mcΔT, where q is the heat absorbed, m is the mass of the silver, c is the specific heat capacity of silver, and ΔT is the change in temperature. First, calculate the change in temperature (ΔT = 41.8°C - 33.0°C = 8.8°C). The specific heat capacity of silver is 0.235 J/g°C. Convert the heat from kJ to J (1 kJ = 1000 J). Then, rearrange the formula to solve for the mass (m = q / (cΔT)). Plug in the values and calculate the mass in grams.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.