Can someone please answer this

Question

1. where not met in 200 iterations 

Given the following information for substance X:

Specific Heat (c) of solid phase: 2.0 J/g°C

Heat of Fusion (Lf): 100 J/g

Specific Heat (c) of liquid phase: 5.0 J/g°C

Heat of Vaporization (Lv): 1000 J/g

Specific Heat (c) of vapor phase: 1.0 J/g°C

Calculate the total heat energy in Joules needed to convert 27.1. g of substance X from -2 °C to 48 °C?

Type your answer with 3 sig figs

Answer 1

ΔH₁ = q₁ = mCΔT₁

<=> (27.1g)[2.0 J*(g*C)^-1][5C - (-2C)]

ΔH₁ = q₁ = 378J

ΔH₂ = q₂ = mΔH_fus = mL_f

<=> (27.1g)(100J*C^-1)

ΔH₂ = q₂ = 2710J

ΔH₃ = q₃ = mCΔT₃

<=> (27.1g)[5.0 J*(g*C)^-1](43C - 5C)

ΔH₃ = q₃ = 5826.5J

q_total = q₁ + q₂ + q₃

q_total = 8.91x10³J

Answer 2

From the figure..

melting point = 5ºC

boiling point = 55ºC

For the following calculations, we'll use q, m, C, ∆T, ∆Hf, and ∆Hvap

q = heat

m = mass

C = specific heat

∆T = change in temperature

∆Hf = heat of fusion

∆Hvap = heat of vaporization

Best to answer this type of question in steps.

Step1: heat to convert 27.1 g of solid x from -2º to 5º

q = mC∆T = (27.1 g)(2.0 J/gº)(7º) = 379 J

Step 2: heat to melt 27.1 g of solid x to form a liquid at the melting point. This is just a phase change.

q = m∆Hf = (27.1 g)(100 J/g) = 2710 J

Step 3: heat to raise temperature of liquid x from 5º to 48º

q = mC∆T = (27.1 g)(5.0 J/gº)(43º) = 5827 J

Total all the heat values

379 J + 2710 J + 5827 J = 8916 J = 8920 J (answer to 3 sig. figs.)