Question

A cup of 132 g of water is heated from 30 oC until all of the water changed to water vapor. What amount of energy is required?

Answer 1

q = 336,943.2J

Step-by-step explanation

Given that;

The mass of water is 132 g

The temperature of water is 30 degrees Celcius

Follow the steps below to find the amount of energy required

Step 1; Calculate the heat required to warm water from 30oC to 100oC

`\text{ q = mc}\Delta T`

Substitute the given data into the formula above

`\begin{gathered} \text{ c = 4.18 J/g}\degree C \\ \text{ q}_1\text{ = 132 }*\text{ 4.18}*(100\text{ - 30\rparen} \\ \text{ q}_1\text{ = 132 }*\text{ 4.18 }*\text{ 70} \\ \text{ q}_1\text{ = 38,623.2J} \end{gathered}`

Step 2; Calculate the amount of heat required vapourize the water steam

`\text{ q = m}\Delta H_(vap)`
`\begin{gathered} \text{ }\Delta H_{vap\text{ }}=\text{ 2260J.g}^(-1) \\ \text{ q}_2\text{ = 132}*2260 \\ \text{ q}_2\text{ }=\text{ 298320 J} \end{gathered}`

The total energy is

q = q1 + q2

q = 38,623.2 + 298320

q = 336,943.2J