How much energy must a stove transfer to completely heat 1g of liquid water from 1o C to 25o C?

The energy needed by a stove to transfer heat completely to 1 g of liquid water fro 1 °C to 25 °C is 100.37 J.What is energy?Energy is the ability or the capacity to do work.To calculate the  amount of energy, we use the formula below.Formula:Q = cm(t₂-t₁).............. Equation 1Where:Q = Amount of energyc = Specific heat capacity of the waterm = mass of the watert₂ = Final temperaturet₁ = Initial temperatureFrom the question,Given:m = 1 g = 0.001 kgc = 4182 J/kg°Ct₁ = 1 °Ct₂ = 25 °CSubstitute these values into equation 1Q = 0.001(4182)(25-1)Q = 100.37 JHence, The energy required is 100.37 J.Learn more about energy here: https://brainly.com/question/19666326#SPJ1

Taking into account the definition of calorimetry, the energy that a stove must transfer to completely heat 1 g of liquid water from 1 °C to 25 °C is 100.416 J.Definition of calorimetryCalorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.When heat added or removed from a substance causes a temperature change in it without affecting its molecular structure, it is called sensible heat.So, the expression that allows to calculate heat exchanges is:Q = c× m× ΔTwhere:Q is the heat exchanged by a body of mass m.c is the specific heat substance.ΔT is the temperature variation.Energy in this caseIn this case, you know:Q= ?c= 4.184 J/gCm= 1 gΔT= Tfinal - Tinitial= 25 C - 1 C= 24 CReplacing in the definition of calorimetry:Q = 4.184 J/gC× 1 g× 24 CSolving: Q= 100.416 JFinally, the energy needed is 100.416 J.Learn more about calorimetry:brainly.com/question/13830016brainly.com/question/14549135#SPJ1