What amount of heat is needed to raise 27.0 g of water from 10.0 °C to 90.0 °C?

Answer 1

A heat of 9.04 kJ is required.

The equation to apply is

#q = mcΔT#
where #q# is the heat, #m# is the mass, #c# is the specific heat capacity, and #ΔT# is the temperature change.
#m# = 27.0 g; #c# = 4.184 J·°C⁻¹g⁻¹; #ΔT = T_2 - T_1# = (90.0 – 10.0) °C = 80.0°C
#q = mcΔT# = 27.0 g × 4.184 J·°C⁻¹g⁻¹ × 80.0 °C = 9040 J = 9.04 kJ
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Answer 2

The amount of heat needed is 6081 J.

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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.

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.

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.

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.

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