How much energy must be supplied to change 36 g of ice at 0° C to water at room temperature 25° C ? Data for water Δ Hf u s i o no text6 text.01 textkJ/mol ( textC) textp text(liquid) text4 text.18 textJK- text1 textg- text1

Question

How much energy must be supplied to change 36 g of ice at 0° C to water at room temperature 25° C ? Data for water Δ Hf u s i o no text6 text.01 textkJ/mol ( textC) textp text(liquid) text4 text.18 textJK- text1 textg- text1 (A) 12 kJ (B) 16 kJ (C) 19 kJ (D) 22 kJ

Tardigrade Admin · Accepted Answer

Δ H=(.Δ Hf u s i o n.) of two moles +msΔ t =6.01× 2+36× 4.18× 25× 10- 3 = 16 kJ.

Data for water
$Δ H_{f u s i o n}^{o}$	$6 .01 kJ/mol$
$(C)_{p (liquid)}$	$4 .18 JK^{- 1} g^{- 1}$

Q. How much energy must be supplied to change 36 g of ice at $0^{\circ} C$ to water at room temperature $2 5^{\circ} C$ ?

Data for water

$Δ H_{f u s i o n}^{o}$
$6 .01 kJ/mol$

$(C)_{p (liquid)}$
$4 .18 JK^{- 1} g^{- 1}$

12 kJ

16 kJ

19 kJ

22 kJ

$Δ H = (Δ H_{f u s i o n})$ of two moles $+ m s Δ t$
$= 6.01 \times 2 + 36 \times 4.18 \times 25 \times 1 0^{- 3}$
= 16 kJ.

Q. How much energy must be supplied to change 36 g of ice at 0∘C to water at room temperature 25∘C ? Data for water ΔHfusiono​ 6.01kJ/mol (C)p(liquid)​ 4.18JK−1g−1