Question

In order to make 4 cups of tea, 1.00 kg of water is heated from 22.0 oC to 99.0 oC. How much energy is required? 1) One point for how you would set up the problem and correct answer 2) 1 point for explaining any conversions 3) One point for explaining if this is endothermic or exothermic and why

Answer 1

To heat 1 kg of water from 22.0 oC to 99.0 oC, 323,008 J of energy is required.

Step-by-step explanation:

To determine the amount of energy required to heat 1 kg of water from 22.0 oC to 99.0 oC, we need to use the equation Q = mcΔT, where Q is the energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

Given that the water has a specific heat capacity of 4.184 J/g °C, we can convert the mass of 1.00 kg of water to grams by multiplying by 1000, resulting in 1000 g. Additionally, we can calculate the change in temperature by subtracting the initial temperature from the final temperature, which gives us ΔT = 99.0 oC - 22.0 oC = 77.0 oC.

Plugging these values into the equation, we have Q = (1000 g)(4.184 J/g °C)(77.0 oC) = 323,008 J. Therefore, the amount of energy required to heat 1.00 kg of water from 22.0 oC to 99.0 oC is 323,008 J.

Answer 2

`322014\ \text{J}`

Step-by-step explanation:

m = Mass of water = 1 kg

c = Specific heat of water =
`4182\ \text{J/kg}^(\circ)\text{C}`

`\Delta T` = Change in temperature =
`(99-22)^(\circ)\text{C}`

Heat or energy required in the system is

`Q=mc\Delta T\\\Rightarrow Q=1* 4182* (99-22)\\\Rightarrow Q=322014\ \text{J}`

The energy required is
`322014\ \text{J}`

Unit of energy is Joule

`mc\Delta T=\text{kg}* \frac{\text{J}}{\text{kg}^(\circ)\text{C}}*\ ^(\circ)\text{C}=\text{J}`

As heat is being absorbed by the water it is endothermic in nature.