How much energy does it take to heat 346 g of steam at 100 degrees to steam at 110 degrees Celsius if the specific heat of steam is 2.01 J/g°C?

Question

Luna Chen · Accepted Answer

Use The Thermochem Equation

#q=mcDeltat# Where: #q# = energy used/gained #m# =mass of system being heated/cooled #Deltat# =temp. change #c# = specific heat capacity Based on the information given, we can calculate the #Deltat#: #Deltat# = final temp - initial temp #Deltat = 110 - 100# #Deltat = 10°C# We also know that: #m# = 346 g #c# = 2.01 J/g°C So we can now sub everything into our equation: #q=mcDeltat# #q#=(346g)(2.01J/g°C)(10°C) #q# = 6954.6 J

Wyatt Atkins · Answer

undefined To calculate the energy required to heat 346 g of steam from 100°C to 110°C, you can use the formula:

Energy = mass × specific heat capacity × temperature change

First, find the temperature change:
ΔT = final temperature - initial temperature
ΔT = 110°C - 100°C
ΔT = 10°C

Then, use the formula:
Energy = 346 g × 2.01 J/g°C × 10°C

Calculate the energy:
Energy = 346 g × 2.01 J/g°C × 10°C = 6954.6 J

So, it takes 6954.6 Joules of energy to heat 346 g of steam from 100°C to 110°C.